General Questions and Answers

4 Al (s) + 3 02 (g)
Answer:
-
2 Al2O3 (s)
How many grams of Al (s) are needed to produce 197.8 g of Al2O3 if the percent yield for this reaction is 83.2% ? Assume that oxygen is present in excess.
Do NOT include units in your answer. If you round during your calculation, be sure to keep at least three (3) decimal places. Report your answer to one (1) decimal places.
Physical Chemistry
General
4 Al (s) + 3 02 (g) Answer: - 2 Al2O3 (s) How many grams of Al (s) are needed to produce 197.8 g of Al2O3 if the percent yield for this reaction is 83.2% ? Assume that oxygen is present in excess. Do NOT include units in your answer. If you round during your calculation, be sure to keep at least three (3) decimal places. Report your answer to one (1) decimal places.
Drag each item to the correct box.
Rank the following atoms in order of increasing electronegativity.
least electronegative
N
most electronegative
Physical Chemistry
General
Drag each item to the correct box. Rank the following atoms in order of increasing electronegativity. least electronegative N most electronegative
Identify which sets of chemical reactions resulted in a white precipitate.
(HINT: Please refer to the completed chart that you filled out during the hands-on
lab OR the virtual video lab. You will need to look for the chemical sets that
provided the color of precipitate listed above.)
Select 3 correct answer(s)
BaCl2 + AgNO3
Al2(SO4)3 + Ba(NO3)2
BaCl2 + KCI
Na2CrO4 + AgNO3
BaCl2 + K₂CRO4
BaCl2 + MgSO4
Physical Chemistry
General
Identify which sets of chemical reactions resulted in a white precipitate. (HINT: Please refer to the completed chart that you filled out during the hands-on lab OR the virtual video lab. You will need to look for the chemical sets that provided the color of precipitate listed above.) Select 3 correct answer(s) BaCl2 + AgNO3 Al2(SO4)3 + Ba(NO3)2 BaCl2 + KCI Na2CrO4 + AgNO3 BaCl2 + K₂CRO4 BaCl2 + MgSO4
When the Roman Empire could no
longer expand, what did it do to
increase revenue for the
government?
A. It acquired more slaves from other parts of
the world.
B. It sells the land back to the barbarians.
C. It taxes the citizens.
D. It forced those that were not citizens to leave
the empire.
Physical Chemistry
General
When the Roman Empire could no longer expand, what did it do to increase revenue for the government? A. It acquired more slaves from other parts of the world. B. It sells the land back to the barbarians. C. It taxes the citizens. D. It forced those that were not citizens to leave the empire.
How many grams of Al are need to react with 3.4 mol HCl?
Given that 2 Al + 6 HCl → 2 AlCl3 + 3H₂
0 25g
O 15 g
O 93 g
O 1.1 g
O 31 g
O 275 g
O 26 g
Physical Chemistry
General
How many grams of Al are need to react with 3.4 mol HCl? Given that 2 Al + 6 HCl → 2 AlCl3 + 3H₂ 0 25g O 15 g O 93 g O 1.1 g O 31 g O 275 g O 26 g
What is the wavelength of the matter wave associated with a proton moving at 315 m/s?
wavelength of proton matter wave:
wavelength of astronaut matter wave:
What is the wavelength of the matter wave associated with a 155 kg astronaut (including her spacesuit) moving at the
same speed?
125 x10
0-11
wavelength of Earth matter wave:
x10
What is the wavelength of the matter wave associated with Earth moving along its orbit around the Sun?
x10
m
m
m
Physical Chemistry
General
What is the wavelength of the matter wave associated with a proton moving at 315 m/s? wavelength of proton matter wave: wavelength of astronaut matter wave: What is the wavelength of the matter wave associated with a 155 kg astronaut (including her spacesuit) moving at the same speed? 125 x10 0-11 wavelength of Earth matter wave: x10 What is the wavelength of the matter wave associated with Earth moving along its orbit around the Sun? x10 m m m
Avobenzone is an active ingredient in some common sunscreens. Which of the following is the correct molecular formula for avobenzone?
solla
avobenzone
Multiple Choice
C20H2403
C20H2203
C2202203
C21H2303
< Prex
9 of 20
www
www
Next >
55°F Mos
Physical Chemistry
General
Avobenzone is an active ingredient in some common sunscreens. Which of the following is the correct molecular formula for avobenzone? solla avobenzone Multiple Choice C20H2403 C20H2203 C2202203 C21H2303 < Prex 9 of 20 www www Next > 55°F Mos
The balanced reaction equation for combustion of heptane, C₂H16, i
is
C₂H₁6 + 110₂7CO₂ + 8H₂0
If the reaction produced 28.5 g CO₂, how many grams of heptane were burned?
mass:
The reaction of limestone with hydrochloric acid is
CaCO3 + 2HCl → CaCl₂ + CO₂ + H₂O
If the reaction produced 28.5 g CO2, how many grams of HCl reacted?
mass:
g C₂H16
g HCI
Physical Chemistry
General
The balanced reaction equation for combustion of heptane, C₂H16, i is C₂H₁6 + 110₂7CO₂ + 8H₂0 If the reaction produced 28.5 g CO₂, how many grams of heptane were burned? mass: The reaction of limestone with hydrochloric acid is CaCO3 + 2HCl → CaCl₂ + CO₂ + H₂O If the reaction produced 28.5 g CO2, how many grams of HCl reacted? mass: g C₂H16 g HCI
14. Which of the following "rules" is being violated in each electron configuration below? Explain
your answer for each. Hund's Rule, Pauli Exclusion Principle, Aufbau Principle
11
12
13
↑↓ ↑↓ 14.
1s 2s
2p
↑↓ 11 11 14
1s
2s
2p
↑↓ ↑↓ ↑↓↑↑↓
2p
14 1s 2s
-
3s
TL TL ↑↓↑↑↓ ↑↑ ttttt
1s
2s
2p
3s
3p
NIL
3p
↑↓ ↓ ↓ ↓ ↓↓↓↓↓
3s
3p
3d
Physical Chemistry
General
14. Which of the following "rules" is being violated in each electron configuration below? Explain your answer for each. Hund's Rule, Pauli Exclusion Principle, Aufbau Principle 11 12 13 ↑↓ ↑↓ 14. 1s 2s 2p ↑↓ 11 11 14 1s 2s 2p ↑↓ ↑↓ ↑↓↑↑↓ 2p 14 1s 2s - 3s TL TL ↑↓↑↑↓ ↑↑ ttttt 1s 2s 2p 3s 3p NIL 3p ↑↓ ↓ ↓ ↓ ↓↓↓↓↓ 3s 3p 3d
Consider compounds which contain both a heteroatom and a double bond. For which compound is no additional Lewis structure possible?
Multiple Choice
O
||
|||
IV
11
E
|||
IV
Physical Chemistry
General
Consider compounds which contain both a heteroatom and a double bond. For which compound is no additional Lewis structure possible? Multiple Choice O || ||| IV 11 E ||| IV
A mixture of 8 moles of hydrogen and 6 moles of oxygen are used in the reaction.
Use the coefficients from the balanced chemical equation in your calculation.
a) How many moles of water would be produced if you used up all the hydrogen?
[Select]
mol
b) How many moles of water would be produced if you used up all the oxygen?
[Select]
mol
c) Given your answers above and assessing the limiting reactant, how many moles
of water can be produced?
[Select]
mol
d) Which is the limiting reactant? [Select]
e) How many moles of excess reactant is left over?______moles start -
moles used = moles left over
[Select]
mol excess reactant initially - [Select]
mol excess reactant used = [Select]
mol excess reactant left over
Physical Chemistry
General
A mixture of 8 moles of hydrogen and 6 moles of oxygen are used in the reaction. Use the coefficients from the balanced chemical equation in your calculation. a) How many moles of water would be produced if you used up all the hydrogen? [Select] mol b) How many moles of water would be produced if you used up all the oxygen? [Select] mol c) Given your answers above and assessing the limiting reactant, how many moles of water can be produced? [Select] mol d) Which is the limiting reactant? [Select] e) How many moles of excess reactant is left over?______moles start - moles used = moles left over [Select] mol excess reactant initially - [Select] mol excess reactant used = [Select] mol excess reactant left over
A. copper sulfate (CuSO4) solution and steel wool (Fe). (6 pt.)
balanced equation
total ionic equation
net ionic equation
reaction type
B. steel wool (Fe) and sulfur (S8) (4 pt.)
balanced equation
reaction type
Physical Chemistry
General
A. copper sulfate (CuSO4) solution and steel wool (Fe). (6 pt.) balanced equation total ionic equation net ionic equation reaction type B. steel wool (Fe) and sulfur (S8) (4 pt.) balanced equation reaction type
The unbalanced equation above shows carbon and silicon dioxide reacting to form
silicon carbide (SiC, molar mass = 40.1 g/mol) and copper. Balance it before beginning.
Silicon carbide is a semiconductor, and copper is an excellent conductor of electric
current.
Previously cited
A large electronics company is creating and testing SiC for use in new computer chips. A
chemical technician has 22.0 g of each reactant. Assuming a 100% yield, what mass (in
grams) of silicon carbide can be created from what the technician has available?
g Sic
Answer:
Physical Chemistry
General
The unbalanced equation above shows carbon and silicon dioxide reacting to form silicon carbide (SiC, molar mass = 40.1 g/mol) and copper. Balance it before beginning. Silicon carbide is a semiconductor, and copper is an excellent conductor of electric current. Previously cited A large electronics company is creating and testing SiC for use in new computer chips. A chemical technician has 22.0 g of each reactant. Assuming a 100% yield, what mass (in grams) of silicon carbide can be created from what the technician has available? g Sic Answer:
Balance the following equation:
NH4NO3 (s) →→→
N₂ (g) +
_O₂ (g) +______H₂O (1)
• What is the coefficient for water in the balanced chemical equation?
. If you begin with 55.2 g NH4NO3, what is the theoretical yield of water?
g H₂0
• If the percent yield is 82.6 %, what mass of liquid product was actually obtained in the
reaction?
g H₂
Use the included Periodic Table for all molar mass values. Give 3 significant figures
in all answers.
Physical Chemistry
General
Balance the following equation: NH4NO3 (s) →→→ N₂ (g) + _O₂ (g) +______H₂O (1) • What is the coefficient for water in the balanced chemical equation? . If you begin with 55.2 g NH4NO3, what is the theoretical yield of water? g H₂0 • If the percent yield is 82.6 %, what mass of liquid product was actually obtained in the reaction? g H₂ Use the included Periodic Table for all molar mass values. Give 3 significant figures in all answers.
(1pts) is this chemical equation balanced?
P+80₂4PO,
(1pts)
(1pts)
13. If you have 0.38 moles of P how many moles of O₂ would be
needed to react?
14. If you have 0.28 moles of Os how many moles of PO₂ can be
produced?
15. If you produce 8.07 moles of PO₂, how many moles of P, are
required?
(9pts) Stoichiometry (Chemical Calculations)
Choose...
Saved
Physical Chemistry
General
(1pts) is this chemical equation balanced? P+80₂4PO, (1pts) (1pts) 13. If you have 0.38 moles of P how many moles of O₂ would be needed to react? 14. If you have 0.28 moles of Os how many moles of PO₂ can be produced? 15. If you produce 8.07 moles of PO₂, how many moles of P, are required? (9pts) Stoichiometry (Chemical Calculations) Choose... Saved
Boyle's law. Let's return our balloon to the room again, where it's 26°C. Now imagine that you
take an empty 0.500 L plastic pickle jar and gently push the balloon inside the jar: Now screw
on the lid. What will happen to the pressure inside the balloon when you close the lid? (2 pts/
0.4pt each)
(a) Circle the correct words in the parentheses to complete the following sentence.
The pressure in the balloon will (increase/decrease) (slightly/dramatically). In this
experiment (volume/temperature/amount of gas) (is/are) constant.
(b) Write an equation using the information from (a) that compares the initial state of
the balloon and to its final state. P1V1= P2V2
(c) Calculate the new pressure (in torr) using the ideal gas law or the equation written
from your answer in (b). P=?atm
V1=0.500 L
(d) Now explain the change in pressure based on the behavior of the gas
molecules.
Physical Chemistry
General
Boyle's law. Let's return our balloon to the room again, where it's 26°C. Now imagine that you take an empty 0.500 L plastic pickle jar and gently push the balloon inside the jar: Now screw on the lid. What will happen to the pressure inside the balloon when you close the lid? (2 pts/ 0.4pt each) (a) Circle the correct words in the parentheses to complete the following sentence. The pressure in the balloon will (increase/decrease) (slightly/dramatically). In this experiment (volume/temperature/amount of gas) (is/are) constant. (b) Write an equation using the information from (a) that compares the initial state of the balloon and to its final state. P1V1= P2V2 (c) Calculate the new pressure (in torr) using the ideal gas law or the equation written from your answer in (b). P=?atm V1=0.500 L (d) Now explain the change in pressure based on the behavior of the gas molecules.
Refer to Q#4: Draw the Lewis structure for the FCN molecule. As modeled and discussed in the live session:
How many electrons are present in the Lewis Dot Structure for FCN?
O 16
18
O 20
O 14
Physical Chemistry
General
Refer to Q#4: Draw the Lewis structure for the FCN molecule. As modeled and discussed in the live session: How many electrons are present in the Lewis Dot Structure for FCN? O 16 18 O 20 O 14
A student intended to make a salt solution with a concentration of 10.0 grams of
solute per liter of solution. When the student's solution was analyzed, it was
found to contain 8.90 grams of solute per liter of solution. What was the percent
error in the concentration of the solution?
1) 1.10%
2) 8.90%
Experimental value:
Theoretical value:
Percent error =
3) 11.0%
4) 18.9%
Physical Chemistry
General
A student intended to make a salt solution with a concentration of 10.0 grams of solute per liter of solution. When the student's solution was analyzed, it was found to contain 8.90 grams of solute per liter of solution. What was the percent error in the concentration of the solution? 1) 1.10% 2) 8.90% Experimental value: Theoretical value: Percent error = 3) 11.0% 4) 18.9%
When you calculate the density of chemical A experimentally you get 1.13 g/mL. The
actual density according to the literature is 1.16 g.mL. What is your percent error?
Experimental value:
Theoretical value:
Percent error =
Physical Chemistry
General
When you calculate the density of chemical A experimentally you get 1.13 g/mL. The actual density according to the literature is 1.16 g.mL. What is your percent error? Experimental value: Theoretical value: Percent error =
2Mg(s) + O₂(g) →→→ 2MgO(s)
A college chemistry student is performing this reaction in a lab, where magnesium is
burned and combines with oxygen from the air to produce magnesium oxide.
The students burns 2.92 g of Mg, and there is excess oxygen from the air. They
incorrectly calculated that the mass of magnesium oxide produced was 2.42 g. Here is
their work:
2.92 g 1 mol
2 mol
X
X
24.3 g
1 mol
X
40.3 g = 2.42 g
-
1 mol
1) What did the student do wrong? There is an error in their work. Explain specifically
what part is incorrect. (2 pts)
2) What recommendation(s) would you give to the student regarding showing their
work? There is an improvement that can be made to help them avoid this mistake in the
future. (2 pts)
3) Instead of 2.42 g, what answer should the student have gotten? (2 pts)
Physical Chemistry
General
2Mg(s) + O₂(g) →→→ 2MgO(s) A college chemistry student is performing this reaction in a lab, where magnesium is burned and combines with oxygen from the air to produce magnesium oxide. The students burns 2.92 g of Mg, and there is excess oxygen from the air. They incorrectly calculated that the mass of magnesium oxide produced was 2.42 g. Here is their work: 2.92 g 1 mol 2 mol X X 24.3 g 1 mol X 40.3 g = 2.42 g - 1 mol 1) What did the student do wrong? There is an error in their work. Explain specifically what part is incorrect. (2 pts) 2) What recommendation(s) would you give to the student regarding showing their work? There is an improvement that can be made to help them avoid this mistake in the future. (2 pts) 3) Instead of 2.42 g, what answer should the student have gotten? (2 pts)
Phosphorus trichloride is produced by the reaction of phosphorus and chlorine as
shown in the following balanced chemical equation. P4 (s) + 6 Cl₂ (g) → 4 PC13 (1)
Consider the reaction of 125 g P4 and 322 g Cl₂.
1. Determine the maximum amount of PC13 that can be formed from the mass of P4 (in
grams).
g PC13 to 3 SF
2. Determine the maximum amount of PC13 that can be formed from the mass of Cl₂ (in
grams).
g PC13 to 3 SF
3. Based on your answers above, what mass of PC13 is expected to form?
g PCI; to 3 SF
4. What is the limiting reactant?
blank)
5. How much excess reactant (in grams) is left at the end of the reaction?
• Start - used=left over (put numbers in blanks in this order)
g to start with -
O
(write phosphorus or chlorine in the
g used in the reaction =
g left over at the end of the reaction.
6. If the percent yield is 84.5 %, what mass of PC13 was obtained in the reaction
(actual yield)?
g PC13 to 3 SF
Physical Chemistry
General
Phosphorus trichloride is produced by the reaction of phosphorus and chlorine as shown in the following balanced chemical equation. P4 (s) + 6 Cl₂ (g) → 4 PC13 (1) Consider the reaction of 125 g P4 and 322 g Cl₂. 1. Determine the maximum amount of PC13 that can be formed from the mass of P4 (in grams). g PC13 to 3 SF 2. Determine the maximum amount of PC13 that can be formed from the mass of Cl₂ (in grams). g PC13 to 3 SF 3. Based on your answers above, what mass of PC13 is expected to form? g PCI; to 3 SF 4. What is the limiting reactant? blank) 5. How much excess reactant (in grams) is left at the end of the reaction? • Start - used=left over (put numbers in blanks in this order) g to start with - O (write phosphorus or chlorine in the g used in the reaction = g left over at the end of the reaction. 6. If the percent yield is 84.5 %, what mass of PC13 was obtained in the reaction (actual yield)? g PC13 to 3 SF
How many grams of Al2O3 can form from 38.8 g of Al?
4 Al(s) + 3 O₂(g) → 2 Al₂O3(s)
Step 1: Show the strategy for solving this problem.
grams Al
->
grams Al₂O3
Physical Chemistry
General
How many grams of Al2O3 can form from 38.8 g of Al? 4 Al(s) + 3 O₂(g) → 2 Al₂O3(s) Step 1: Show the strategy for solving this problem. grams Al -> grams Al₂O3
For the following reaction, 14.9 grams of sulfur are allowed to react with 17.3 grams of carbon monoxide.
sulfur (s) + carbon monoxide (g)-sulfur dioxide (g) + carbon (s)
What is the maximum amount of sulfur dioxide that can be formed?
What is the FORMULA for the limiting reagent?
What amount of the excess reagent remains after the reaction is complete?
grams
grams
Physical Chemistry
General
For the following reaction, 14.9 grams of sulfur are allowed to react with 17.3 grams of carbon monoxide. sulfur (s) + carbon monoxide (g)-sulfur dioxide (g) + carbon (s) What is the maximum amount of sulfur dioxide that can be formed? What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams grams
How many grams of Cl₂ are needed to form 79.7 g of AICI, ?
2 Al(s) + 3 Cl₂(g) ->>
2 AICI, (s)
Step 1: Show the strategy for solving this problem.
grams AlCl3
-
grams Cl₂
Physical Chemistry
General
How many grams of Cl₂ are needed to form 79.7 g of AICI, ? 2 Al(s) + 3 Cl₂(g) ->> 2 AICI, (s) Step 1: Show the strategy for solving this problem. grams AlCl3 - grams Cl₂
A molecular compound has the following empirical formula: CH₂O. The molar mass of the empirical formula is
g. Write your answer using 3 significant figures.
If the molar mass of the molecular compound is 180.0 g/mol, write the molecular formula of the compound.
Physical Chemistry
General
A molecular compound has the following empirical formula: CH₂O. The molar mass of the empirical formula is g. Write your answer using 3 significant figures. If the molar mass of the molecular compound is 180.0 g/mol, write the molecular formula of the compound.
Based on periodic trends, which element below has the greatest electronegativity?
O Potassium (K)
O Fluorine (F)
O Bromine (Br)
Physical Chemistry
General
Based on periodic trends, which element below has the greatest electronegativity? O Potassium (K) O Fluorine (F) O Bromine (Br)
Write the molecular and net ionic equations, including phases, for the reaction that occurs between aqueous sodium chloride,
NaCl, and aqueous silver nitrate, AgNO3.
molecular equation:
net ionic equation:
Physical Chemistry
General
Write the molecular and net ionic equations, including phases, for the reaction that occurs between aqueous sodium chloride, NaCl, and aqueous silver nitrate, AgNO3. molecular equation: net ionic equation:
PC15 (s) + H₂O(1) POCl3 (1) + 2HCl(aq)
When 58.15 g of phosphorus pentachloride reacts with excess water, what mass of
hydrogen chloride will be produced?
If needed, enter scientific notation with the "e". For example, 1.44x107 would be entered as
1.44e7.
Answer:
g HCI.
Physical Chemistry
General
PC15 (s) + H₂O(1) POCl3 (1) + 2HCl(aq) When 58.15 g of phosphorus pentachloride reacts with excess water, what mass of hydrogen chloride will be produced? If needed, enter scientific notation with the "e". For example, 1.44x107 would be entered as 1.44e7. Answer: g HCI.
The hydrides of group 5A are NH3, PH3, AsH3, and SbH3. Arrange them from highest to lowest boiling point.
Rank the molecules from highest to lowest boiling point. To rank items as equivalent, overlap them.
View Available Hint(s)
PH3
NH3
SbH3
AsH3
Physical Chemistry
General
The hydrides of group 5A are NH3, PH3, AsH3, and SbH3. Arrange them from highest to lowest boiling point. Rank the molecules from highest to lowest boiling point. To rank items as equivalent, overlap them. View Available Hint(s) PH3 NH3 SbH3 AsH3
Indicate the major type of intermolecular forces between particles in each of the following compounds.
Drag the appropriate items to their respective bins.
Dipole-dipole attractions
NH3
HBr OBr2
CHCl3
Dispersion forces
CF4
Hydrogen bonds
lonic bonds
LICI
Reset Help
Physical Chemistry
General
Indicate the major type of intermolecular forces between particles in each of the following compounds. Drag the appropriate items to their respective bins. Dipole-dipole attractions NH3 HBr OBr2 CHCl3 Dispersion forces CF4 Hydrogen bonds lonic bonds LICI Reset Help
Select the correct answer.
Which reaction is a decomposition reaction?
OA. 2KCIO3- 2KCI +30₂
4Na + O₂ → 2Na₂O
ZnS +30₂
ZnS
+ 30₂ → 2ZnO + 250₂
2NaBr + CaF₂ → 2NaF + CaBr₂
B.
O C.
O D.
Physical Chemistry
General
Select the correct answer. Which reaction is a decomposition reaction? OA. 2KCIO3- 2KCI +30₂ 4Na + O₂ → 2Na₂O ZnS +30₂ ZnS + 30₂ → 2ZnO + 250₂ 2NaBr + CaF₂ → 2NaF + CaBr₂ B. O C. O D.
You are given the number of grams of compound NO₂ and are
asked to determine the number of mol in the sample Choose
the respond that best describes what is needed to solve this
problem.
a. the g of NO₂
sample is
divided by
the molar
mass of NO2
in g/mol
Ob. the molar
mass of NO₂
in g/mol is
divided by the
grams NO₂ in
the sample
O c. the mol of NO₂
is multiplied by
the molar mass
of NO₂ in
g/mol
2 points
Physical Chemistry
General
You are given the number of grams of compound NO₂ and are asked to determine the number of mol in the sample Choose the respond that best describes what is needed to solve this problem. a. the g of NO₂ sample is divided by the molar mass of NO2 in g/mol Ob. the molar mass of NO₂ in g/mol is divided by the grams NO₂ in the sample O c. the mol of NO₂ is multiplied by the molar mass of NO₂ in g/mol 2 points
Calculate the number of pounds of CO₂ released into the atmosphere when a 17.0 gallon tank of gasoline is burned in an
automobile engine. Assume that gasoline is primarily octane, Cg H₁g, and that the density of gasoline is 0.692 g mL-¹. This
assumption ignores additives. Also, assume complete combustion.
Physical Chemistry
General
Calculate the number of pounds of CO₂ released into the atmosphere when a 17.0 gallon tank of gasoline is burned in an automobile engine. Assume that gasoline is primarily octane, Cg H₁g, and that the density of gasoline is 0.692 g mL-¹. This assumption ignores additives. Also, assume complete combustion.
With respect to membrane transport,
diffusion driven transport requires no external energy
active transport always moves at least one molecule with a concentration gradient
O ATP is the only source of energy for active transport
O all of the above are true
O none of the above are true
Physical Chemistry
General
With respect to membrane transport, diffusion driven transport requires no external energy active transport always moves at least one molecule with a concentration gradient O ATP is the only source of energy for active transport O all of the above are true O none of the above are true
Indicate whether or not a precipitate forms when aqueous solutions of the following soluble
compounds are mixed. If a precipitate forms, write the net ionic equation for the reaction.
A precipitate is formed for products that are insoluble and slightly soluble.
a) Na₂S and Sr(NO3)2
b) NH4NO3 and NaBr
c) KCl and NaCl
d) K₂SO4 and Bal₂
Physical Chemistry
General
Indicate whether or not a precipitate forms when aqueous solutions of the following soluble compounds are mixed. If a precipitate forms, write the net ionic equation for the reaction. A precipitate is formed for products that are insoluble and slightly soluble. a) Na₂S and Sr(NO3)2 b) NH4NO3 and NaBr c) KCl and NaCl d) K₂SO4 and Bal₂
How many molecules of NH Br are in 3.746 g of NH Br?
Show the conversions required to solve this problem and calculate the molecules of NH Br.
3.746 g NH Br x
amount of NH Br
=
1 mol NH Br
Answer Bank
6.022 x 1023 molecules NH Br
= ? molecules NH Br
1 mol NH₂ Br
97.94 g NH₂ Br
molecules NH Br
Physical Chemistry
General
How many molecules of NH Br are in 3.746 g of NH Br? Show the conversions required to solve this problem and calculate the molecules of NH Br. 3.746 g NH Br x amount of NH Br = 1 mol NH Br Answer Bank 6.022 x 1023 molecules NH Br = ? molecules NH Br 1 mol NH₂ Br 97.94 g NH₂ Br molecules NH Br
This activity will help you begin balancing simple chemical equations.
Five of the spaces below will have NO number on them. This means that those spaces
each hold an invisible ONE.
Remember, in a balanced chemical equation, there are equal numbers of each atom on
each side of the arrow. Good luck!
1) Zn+0₂ → _ZnO
2) ____ HI →
-
3)____B +_ F₂ → ___ BF3
-
5)__ Fe +
H₂ + 1₂
4)__N+ _H,> _NH,
_H₂ →
—
H₂O → Fe3O4 +
-
——
H₂
Physical Chemistry
General
This activity will help you begin balancing simple chemical equations. Five of the spaces below will have NO number on them. This means that those spaces each hold an invisible ONE. Remember, in a balanced chemical equation, there are equal numbers of each atom on each side of the arrow. Good luck! 1) Zn+0₂ → _ZnO 2) ____ HI → - 3)____B +_ F₂ → ___ BF3 - 5)__ Fe + H₂ + 1₂ 4)__N+ _H,> _NH, _H₂ → — H₂O → Fe3O4 + - —— H₂
3. Which of the following describes the relationship between Jim Crow
and Plessy v. Ferguson?
O A
Jim Crow segregation laws compelled Plessy to protest segregated
trains.
OB Jim Crow segregation laws were made possible by the Plessy v.
Ferguson decision.
OC
OD Plessy v. Ferguson made Jim Crow laws widely accepted, but not
officially legal.
Plessy v. Ferguson hoped to end the segregation common during
Jim Crow.
Physical Chemistry
General
3. Which of the following describes the relationship between Jim Crow and Plessy v. Ferguson? O A Jim Crow segregation laws compelled Plessy to protest segregated trains. OB Jim Crow segregation laws were made possible by the Plessy v. Ferguson decision. OC OD Plessy v. Ferguson made Jim Crow laws widely accepted, but not officially legal. Plessy v. Ferguson hoped to end the segregation common during Jim Crow.
Where is the lanthanide series located?
far left side of the periodic table
far right side of the periodic table
O in the middle of the periodic table
underneath the main section of the periodic table
Physical Chemistry
General
Where is the lanthanide series located? far left side of the periodic table far right side of the periodic table O in the middle of the periodic table underneath the main section of the periodic table
Calculate the mass of precipitate formed when aqueous solutions of the following reactants
are mixed, assuming that the reaction goes to completion.
a) 50.0 mL of 0.150 M (NH4)2SO4 and 100. mL of 0.100 M CaBr₂
10.0 mL of 0.525 M NaCl and 20.0 mL of 0.250 M Pb(NO3)2
c) 15.0 mL of 0.235 M Na₂SO3 and 10.0 mL of 0.525 M BaCl₂
b)
Physical Chemistry
General
Calculate the mass of precipitate formed when aqueous solutions of the following reactants are mixed, assuming that the reaction goes to completion. a) 50.0 mL of 0.150 M (NH4)2SO4 and 100. mL of 0.100 M CaBr₂ 10.0 mL of 0.525 M NaCl and 20.0 mL of 0.250 M Pb(NO3)2 c) 15.0 mL of 0.235 M Na₂SO3 and 10.0 mL of 0.525 M BaCl₂ b)
How many grams of AlPO4 are in 5.56 x 1021 molecules of AIPO?
Show the conversions required to solve this problem and calculate the grams of AlPO4.
5.56 x 1021 molecules AlPO4 X
mass AlPO4
=
1 mol AlPO4
1 mol AlPO4
Answer Bank
6.022 x 1023 molecules AIPO4
= ? g AlPO4
121.95 g AIPO4
g AIPO 4
Physical Chemistry
General
How many grams of AlPO4 are in 5.56 x 1021 molecules of AIPO? Show the conversions required to solve this problem and calculate the grams of AlPO4. 5.56 x 1021 molecules AlPO4 X mass AlPO4 = 1 mol AlPO4 1 mol AlPO4 Answer Bank 6.022 x 1023 molecules AIPO4 = ? g AlPO4 121.95 g AIPO4 g AIPO 4
Consider the reaction.
CaCl₂(aq) + K₂CO3(aq) → CaCO3 + 2 KCI
Identify the precipitate, or lack thereof, for the reaction.
O no precipitate
OKCI
O CaCO3
Consider the reaction.
FeCl,(aq) + (NH4),SO4 (aq) — FeSO4 +2NHẠCI
Identify the precipitate, or lack thereof, for the reaction.
O NH CI
no precipitate
O FeSO4
Physical Chemistry
General
Consider the reaction. CaCl₂(aq) + K₂CO3(aq) → CaCO3 + 2 KCI Identify the precipitate, or lack thereof, for the reaction. O no precipitate OKCI O CaCO3 Consider the reaction. FeCl,(aq) + (NH4),SO4 (aq) — FeSO4 +2NHẠCI Identify the precipitate, or lack thereof, for the reaction. O NH CI no precipitate O FeSO4
Suppose you heat a metal object with a mass of 32.9 g to 96.6 °C and transfer it to a calorimeter containing 100.0 g of water at
17.2 °C. The water and metal reach a final temperature of 22.4 °C.
What is the specific heat of the metal inc?
Type answer:
Physical Chemistry
General
Suppose you heat a metal object with a mass of 32.9 g to 96.6 °C and transfer it to a calorimeter containing 100.0 g of water at 17.2 °C. The water and metal reach a final temperature of 22.4 °C. What is the specific heat of the metal inc? Type answer:
Watch the animation and select the interactions that can be explained by hydrogen bonding.
Check all that apply.
View Available Hint(s)
OCH4 molecules interact more closely in the liquid than in the gas phase.
Ice, H₂O, has a solid structure with alternating H-O interactions.
OH₂ Te has a higher boiling point than H₂S.
OHF is a weak acid neutralized by NaOH.
HF has a higher boiling point than HCl.
Physical Chemistry
General
Watch the animation and select the interactions that can be explained by hydrogen bonding. Check all that apply. View Available Hint(s) OCH4 molecules interact more closely in the liquid than in the gas phase. Ice, H₂O, has a solid structure with alternating H-O interactions. OH₂ Te has a higher boiling point than H₂S. OHF is a weak acid neutralized by NaOH. HF has a higher boiling point than HCl.
A chemist dissolves 491. mg of pure barium hydroxide in enough water to make up 170. mL of solution. Calculate the pH of the solution. (The temperature of
the solution is 25 °C.)
Round your answer to 3 significant decimal places.
Physical Chemistry
General
A chemist dissolves 491. mg of pure barium hydroxide in enough water to make up 170. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 3 significant decimal places.
At the start of nerve transmission,
O potassium gates open to attempt to restore the charge imbalance caused by opening of the sodium gates
the first ions to move are protons
the second ion to move is sodium
all of the above are true
4 pts
none of the above are true
Physical Chemistry
General
At the start of nerve transmission, O potassium gates open to attempt to restore the charge imbalance caused by opening of the sodium gates the first ions to move are protons the second ion to move is sodium all of the above are true 4 pts none of the above are true
in Appendix 1 of this lab
write the balanced molecular
equation for each of the precipitation reactions in aqueous solution and the net ionic
equation for the precipitate that is formed. Indicate the phase, (aq), (1), (s), or (g), for each
of the reactants and products. The formation of a precipitate is indicated as a solid, (s). A
precipitate is formed for products that are insoluble and slightly soluble.
a) Ammonium chloride reacts with silver nitrate.
b)
Sodium carbonate reacts with calcium bromide.
c) Barium nitrate reacts with magnesium sulfate.
d) Sodium phosphate (Na3PO4) reacts with lead nitrate (Pb(NO3)2).
Physical Chemistry
General
in Appendix 1 of this lab write the balanced molecular equation for each of the precipitation reactions in aqueous solution and the net ionic equation for the precipitate that is formed. Indicate the phase, (aq), (1), (s), or (g), for each of the reactants and products. The formation of a precipitate is indicated as a solid, (s). A precipitate is formed for products that are insoluble and slightly soluble. a) Ammonium chloride reacts with silver nitrate. b) Sodium carbonate reacts with calcium bromide. c) Barium nitrate reacts with magnesium sulfate. d) Sodium phosphate (Na3PO4) reacts with lead nitrate (Pb(NO3)2).
Balance the equations by inserting coefficients as needed.
equation 1: CaCO3 + HCl
equation 2:
CaCl₂ + CO₂ + H₂O
CaH₂ + H₂O → Ca(OH)₂ + H₂
Physical Chemistry
General
Balance the equations by inserting coefficients as needed. equation 1: CaCO3 + HCl equation 2: CaCl₂ + CO₂ + H₂O CaH₂ + H₂O → Ca(OH)₂ + H₂
Identify which of the following molecules can exhibit hydrogen bonding as a pure liquid.
Check all that apply.
► View Available Hint(s)
F
OF-C-F
I
F
O
H-C-H
H
H
OF-C-H
F
H
N
H
OH-0-0-H
H₂C-H₂C-0-H
OH-Cl
Physical Chemistry
General
Identify which of the following molecules can exhibit hydrogen bonding as a pure liquid. Check all that apply. ► View Available Hint(s) F OF-C-F I F O H-C-H H H OF-C-H F H N H OH-0-0-H H₂C-H₂C-0-H OH-Cl
For an experiment a scientist needs a 0.445 L solution of 0.725 M acetic acid. The labs has a bottle
of 18.3 M concentrated acetic acid. What volume in milliliter (mL) of the concentrated acetic acid
does the scientist need to use to create their solution?
O 17.6 mL
O 0.0176 mL
O 11.2 mL
O 11200 mL
O 29.8 mL
Physical Chemistry
General
For an experiment a scientist needs a 0.445 L solution of 0.725 M acetic acid. The labs has a bottle of 18.3 M concentrated acetic acid. What volume in milliliter (mL) of the concentrated acetic acid does the scientist need to use to create their solution? O 17.6 mL O 0.0176 mL O 11.2 mL O 11200 mL O 29.8 mL