Inorganic Chemistry Questions
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Inorganic Chemistry
Preparation and Properties of CompoundsConsider the reaction:
Br2(g) + Cl₂(g) → 2BrCl(g)
Given an initial mass of 19.86 g Br2, an excess of Cl₂, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of
BrCl produced by the reaction.
Inorganic Chemistry
Qualitative analysisCalculate the mass of gold (III) chloride (Au2Cl6) that contains a million (1.0 × 10^6) chlorine atoms.
Be sure your answer has a unit symbol if necessary, and round it to 2 significant digits.
Inorganic Chemistry
Classification of Elements and PeriodicityConsider the following unbalanced equation:
C2H6(g)+Oz(g)→ CO2(g)+H2O(g)
Which amount requires more oxygen gas, 2.43 mol C₂H6 or 28.8 g C₂H6?
HOW DO WE GET THERE?
For 2.43 mol C₂H6:
What is the mole ratio between C₂H6 and O₂ in the balanced equation?
2C2H6(g) + 702(g) → 4CO2(g) + 6H₂O(g)
X =
Y =
X mol O₂
Y mol C₂H6
mol O₂
mol C₂H6
Inorganic Chemistry
Qualitative analysisCalculate the number of oxygen atoms in a 60.0 g sample of diphosphorus pentoxide (P₂O5).
Be sure your answer has a unit symbol if necessary, and round it to 3 significant digits.
Inorganic Chemistry
S Block - Group 2Hematite, Fe2O3, is an important ore of iron. The free metal is obtained by reacting hematite with carbon monoxide, CO, in a blast furnace. Carbon monoxide is
formed in the furnace by partial combustion of carbon. The reaction is
Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)
How many grams of iron can be produced from 1.62×103 g Fe2O3 reacting with an excess of CO?
HOW DO WE GET THERE?
How many moles are present in 1.62×10³ g of Fe₂O3(s)?
mol Fe2O3(s)
Inorganic Chemistry
Preparation and Properties of CompoundsCalculate the number of oxygen atoms in a 130.0 g sample of dinitrogen tetroxide (N₂O4).
Be sure your answer has a unit symbol if necessary, and round it to 4 significant digits.
Inorganic Chemistry
MetallurgyThis is the chemical formula for nickel tetracarbonyl (a powerfully poisonous liquid used in nickel refining):
Ni(CO)4
A chemical engineer has determined by measurements that there are 4.277 moles of carbon in a sample of nickel tetracarbonyl. How many moles of
oxygen are in the sample?
Round your answer to 4 significant digits.
Inorganic Chemistry
Preparation and Properties of CompoundsCalculate the number of hydrogen atoms in a 80.0 g sample of ammonia (NH3).
Inorganic Chemistry
Qualitative analysisCalculate the number of oxygen atoms in a 80.0 g sample of forsterite (Mg2SiO4).
Be sure your answer has a unit symbol if necessary, and round it to 3 significant digits.
Inorganic Chemistry
Qualitative analysisYou have a solution that is 18.5% (v/v) methyl alcohol. If the bottle contains 1.09 L of solution, what is the volume (V) in milliliters of methyl alcohol?
Express your answer with the appropriate units.
Inorganic Chemistry
Classification of Elements and PeriodicityMeasurements show that unknown compound X has the following composition:
element mass %
nitrogen 26.0%
oxygen 74.1%
Write the empirical chemical formula of X.
Inorganic Chemistry
Qualitative analysisConsider the following unbalanced equation:
C2H6(g) + O2(g) → CO₂(g) + H₂O(g)
Which amount requires more oxygen gas, 2.43 mol C₂H6 or 28.8 g C2H6?
HOW DO WE GET THERE?
For 28.8 g C2H6:
How many moles are present in 28.8 g C₂H6?
mol C₂H6
Inorganic Chemistry
Preparation and Properties of CompoundsMolarity is one of the most commonly used concentration units for
solutions and is abbreviated as "M".
Molarity is calculated by determining the number of moles of the
solute, or the substance being dissolved, in 1 liter of solution. In
other words, molarity is the number of moles/liter. This is
summarized as follows:
Molarity (M)= moles of solute/1 L of solution
What is the molarity of a solution prepared from 34.5 grams of NaCl
in 250.0 milliliters of solution?
0.138 M NaCl
6.78 M NaCl
2.36 M NaCl
0.424 M NaCl
I DON'T KNOW YET
Inorganic Chemistry
Preparation and Properties of CompoundsConsider the following unbalanced equation:
NH3(g) → N₂(g) + H₂(g)
How many moles of N₂ will be produced by the decomposition of 4.06 moles of ammonia?
How many moles of N₂ are produced from 4.06 mol NH3?
mol N₂
Inorganic Chemistry
Qualitative analysisA flask contains 0.015 mol of HCl in 10.0 mL of water.
a. What is the molarity of the HCl solution?
b. In a titration with NaOH, how many moles of NaOH will be required to reach the
end point?
Inorganic Chemistry
Qualitative analysisA 6.00 % (m/v) NaCl solution contains 18.2 g of NaCl. What is the total volume (V) of the solution in
milliliters?
Express your answer with the appropriate units.
Inorganic Chemistry
MetallurgyA solution containing 1.63 g of barium chloride is added to a solution containing 2.40 g of sodium chromate (chromate ion, CrO2). Determine which reactant is in excess. Find the number of grams of barium chromate that can precipitate.
Inorganic Chemistry
Metallurgystrong electrolyte
weak electrolyte
nonelectrolyte
A 20 mL solution containing 2 mmol of HBr(g) was integrated into to a circuit that powers a
light bulb. When the power supply was turned on, the light bulb produced a bright glow.
HBr (g) is a
A 20 mL solution containing 2 mmol of C12H22O11 (aq) was integrated into to a circuit that
powers a light bulb. When the power supply was turned on, the light bulb remained off.
C12H22O11 (aq) is a
A 20 mL solution containing 2 mmol of Ca3(PO4)2 (s) was integrated into to a circuit that
powers a light bulb. When the power supply was turned on, the light bulb faintly flickered.
Ca3(PO4)2 (s) is a
A 20 mL solution containing 2 mmol of CH3NH₂(1) was integrated into to a circuit that
powers a light bulb. When the power supply was turned on, the light bulb produced a dim glow.
CH3NH₂(l) is a
Inorganic Chemistry
Qualitative analysisFor the following reaction, 9.37 grams of glucose (C6H12O6) are allowed to react with 13.6 grams of oxygen gas.
glucose (C6H12O6)(s) + oxygen(g) → carbon dioxide(g) + water(l)
What is the maximum amount of carbon 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?
Inorganic Chemistry
Coordination compoundsConsider the following fictional element and polyatomic ions:
Tb = tiberium (a "complex" transition metal, i.e. forms type II ionic compounds)
TbO2- = tiberite
TbO3- = tiberate
What would be the name of the following compounds:
Tbo tiberium (II)
HTbO3
HTbO2
HTbO
Inorganic Chemistry
Classification of Elements and PeriodicityWhat did Ernest Rutherford discover
and what were there charges?
He discovered the nucleus contained
electrons.
He discovered the nucleus contained
protons.
The electrons possessed a negative
charge.
The protons possessed a positive
charge.
Inorganic Chemistry
Preparation and Properties of CompoundsFor the following reaction, 5.23 grams of nitrogen gas are allowed to react with 9.15 grams of oxygen gas.
nitrogen (g) + oxygen(g) ---> nitrogen monoxide(g)
What is the maximum mass of nitrogen monoxide that can be formed?
What is the FORMULA for the limiting reagent?
What mass of the excess reagent remains after the reaction is complete?
Inorganic Chemistry
Preparation and Properties of Compounds"In our bodies, sugar is broken down with oxygen to produce water and carbon dioxide." According to the following reaction:
C6H12O6 (s) + 6O₂ (g) → 6CO2 (g) + 6H₂O (l)
What would you multiply "moles of glucose (C6H1206)" by to convert to the units "moles of water"?
Inorganic Chemistry
Preparation and Properties of CompoundsFor the following reaction, 25.7 grams of sulfur dioxide are allowed to react with 5.54 grams of oxygen gas.
sulfur dioxide (g) + oxygen (g) → sulfur trioxide (g)
What is the maximum amount of sulfur trioxide that can be formed?
What is the FORMULA for the limiting reagent?
What amount of the excess reagent remains after the reaction is complete?
Inorganic Chemistry
Preparation and Properties of CompoundsInterpret the following equation for a chemical reaction using the coefficients given:
C₂H4(g) + Br2(g) CH₂BrCH₂Br(g)
On the particulate level:
of C₂H4(g) reacts with of Br2(g) to form of CH₂BrCH₂Br(g).
On the molar level:
of C₂H4(g) reacts with of Br2(g) to form of CH₂BrCH₂Br(g).
Inorganic Chemistry
Preparation and Properties of CompoundsDetermine the ionic compound that forms between the given elements.
a. Calcium and chlorine
b. Potassium and iodine
c. Aluminum and sulfur
d. Cesium and nitrogen
e. Magnesium and nitrogen
f. Aluminum and phosphorus
g. Zinc and chlorine
h. Silver and bromine
Inorganic Chemistry
Classification of Elements and PeriodicityWhich of the following are properties of alkali metals?
mostly solids, dull, brittle reactive, conductors
mostly solids, luster, high density, conductors
mostly gases, brittle, dull, low density, insulators
solids, luster, malleable, conductors, reactive
Inorganic Chemistry
Preparation and Properties of CompoundsName the following compounds:
(a) NaH
(b) KMnO4
(c) Ag₂CO3
(d) LizN
Inorganic Chemistry
Preparation and Properties of CompoundsGiven that the following reaction is a precipitation reaction, find the precipitate and the filtrate respectively? 2AgNO3(aq) + CaCl₂(aq) → 2AgCl (s)+ Ca(NO3)2 (aq)
A. CaCl2, Ca(NO3)2-
B. AgCl, Ca(NO3)2-
C. CaCl2, Ca(NO3)2-
D. AgNO3, CaCl2.
Inorganic Chemistry
Preparation and Properties of Compounds(2 points) Phosphonic acid (H3PO3), also known as phosphorous acid, is a diprotic acid. Infrared spectroscopy and nuclear magnetic resonance results indicate that its structure is consistent with the formula OPH(OH)2. With this information, write the correct Lewis structure.
Inorganic Chemistry
Preparation and Properties of CompoundsThe rusting of iron is represented by the equation: 4Fe +302 --> 2Fe₂O3 If you have a 1.45-mol sample of iron, how many moles of Fe₂O3 will there be after the iron has rusted completely?
0.483 mol
2.175 mol
0.967 mol
0.725 mol
1.45 mol
Inorganic Chemistry
Preparation and Properties of CompoundsRefer to the following equation: 4 NH3 (g) + 7 O₂ (g) --> 4 NO₂ (g) + 6 H₂O(g)
How many moles of ammonia will be required to produce 11.9 mol of water?
11.9 mol
5.95 mol
7.93 mol
4.76 mol
none of these options
Inorganic Chemistry
Preparation and Properties of CompoundsBalance the equation below using the smallest possible whole-number stoichiometric coefficients. For the balanced equation, what is the coefficient in front of the reactant O2?
C3H6O + O2 -> CO2 + H2O
Inorganic Chemistry
Preparation and Properties of CompoundsThe sun supplies about 1.1 kilowatt(s) of energy for each square meter of surface area (1.1 kW/m², where a watt = 1 J/s). Plants produce the equivalent of about 0.22 g of sucrose ( C12 H22 O11) per hour per square meter.
12CO2 (g) + 11H₂O (1)→C12H22O11 + 1202 (g) ΔH = 5645kJ
Express your answer using two significant figures.
Inorganic Chemistry
Preparation and Properties of CompoundsConsider the following chemical reaction:
4 NH3 + 7O2 -> 2 N₂O4 + 6H₂O
Identify the limiting reagent when 6.25 mol of NH3 reacts with 10.3 mol of O2.
Assume the reaction goes to completion.
Select one:
O2
NO2
H₂O
NH3
Both NH3 and O2 are used up at the same time
Inorganic Chemistry
MetallurgyIn two or more complete sentences, describe how one of the occupations that you studied would use descriptive statistics when performing their job. Justify your answers in two or more complete sentences.
Inorganic Chemistry
Preparation and Properties of CompoundsThe ionization energy of sodium is 496 kJ/mol. What is the minimum frequency of light required to ionize one electron from one atom of sodium?
2.56 x 10^14 S^-1
6.31 x 10^15 S^-1
3.88 x 10^14 S^-1
8.63 x 10^13 S^-1
1.24 x 10^15 S^-1
Inorganic Chemistry
Classification of Elements and PeriodicityWhat is the electrostatic potential energy (in joules) between an electron and a proton that are separated by 45 pm?
Inorganic Chemistry
Qualitative analysisDoes a reaction occur when aqueous solutions of calcium chloride and ammonium sulfate are combined?
yes/no
If a reaction does occur, write the net ionic equation.
Inorganic Chemistry
Preparation and Properties of CompoundsIn the manufacture ofr NaOH by electrolysis of an aqueous solution of sodium chloride, the cathode and anode are separated by using a diaphragm or slate partitions because
it increases the yield of Cl2
it prevents the reaction taking place between NaOH and Cl₂
it prevents the mixing of NaOH and NaCl
it prevents the reaction taking place between Na and Cl2
Inorganic Chemistry
Preparation and Properties of CompoundsUsing the combined gas law, we solve for P2 by multiplying both sides by _______dividing both sides by _________
The expression obtained is P1V1/T1 x _____ = P2V2 x _____
Finally, P₂ = P₁ x _____
Inorganic Chemistry
MetallurgyA metallurgist has one alloy containing 44 % aluminum and another containing 70 % aluminum. How many pounds of each alloy must he use to make 48 pounds of a third alloy containing 64 % aluminum? (Round to two decimal places if necessary.)
Inorganic Chemistry
S Block - Group 2Which of the following property of magnesium does not resemble with lithium?
Bicarbonates of both exist in solution state but not in solidform
Carbonates of both produce CO₂ on heating
Both can produce nitride on reaction with N₂
Both can be identified by flame colour test
Inorganic Chemistry
Qualitative analysisDoes a reaction occur when aqueous solutions of barium nitrate and magnesium sulfate are combined?
yes / no
If a reaction does occur, write the net ionic equation.
Inorganic Chemistry
Preparation and Properties of CompoundsThe density of titanium is 4.50 g/cm³. A pure titanium cube contains 8.96x 10^23 atoms. What is the edge length of this cube in cm? Provide answer to the correct number of significant figures.
Inorganic Chemistry
Preparation and Properties of CompoundsFor the molecular compound sulfur dioxide, what would you multiply "grams of SO₂ " by to get the units "molecules of SO₂ " ?
Inorganic Chemistry
Preparation and Properties of CompoundsDecide whether each pair of elements in the table below will form an ionic compound. If they will, write the empirical formula and name of the compound formed in the spaces provided.
Inorganic Chemistry
Qualitative analysisIn the photoelectric effect experiment, light shines on a metal and no electrons are emitted from its surface. Which of the following changes might result in electrons
emitted from the metal surface? Check all that apply.
Use light of the same frequency but with higher intensity (brighter).
Use light of a lower wavelength.
Use a different metal surface with a metal having lower binding energy.
Use light of a lower frequency.
Inorganic Chemistry
Qualitative analysisA certain gas is present in a 13.0 L cylinder at 4.0 atm pressure. If the pressure is increased to 8.0 atm, the volume of the gas decreases to 6.5 L. Find the two constants k₁, the initial value of k, and ke, the final value of k, to verify whether the gas obeys Boyle's law. Express your answers to two significant figures separated by a comma.