General Questions and Answers

If 0.850 g of glucose are burned in a bomb calorimeter, the temperature of the 700. g of water in the calorimeter increases from 15.30 °C to 19.00 °C. If the heat capacity of the calorimeter is 660 J/°C what is the value of q for the combustion of the glucose sample? Use Cwater = 4.184J/g °C Report your answer using three significant figures.

State what would happen to red blood cells if placed in a 5% glucose solution? hypotonic hypertonic crenation hemolysis no change

A system releases heat to the surroundings and no work is done on or by the system. What are the signs of system and Select the correct answer below: O system <0 and Wsystem > 0 system > 0 and Wsystem > 0 O 9system >0 and Wsystem = 0 O 9system <0 and Wsystem = 0 FEEDBACK

3.0 mol PbS Express your answer using two significant figures. V= Submit Part B AΣO V = Request Answer Express your answer using two significant figures. VAE ESSAY ? ? mol PbO mol SO₂

Drag each tile to the correct box to create matched pairs. Match the historical events with their effects. spread the Greek culture to Asia caused the beginning of a Jewish diaspora Columblan Exchange conquests by Romans conquests by Alexander the Great led to an exchange of goods between Europe and the Americas

A subunit of an organic compound that confers particular chemical and physical properties is termed. Select one: a. a monomer. b. an oligomer. c. a functional group. d. a synthetic unit. e. an isomer.

8. Fill in the following table, converting the following number of atoms to moles and moles to atoms as needed. (3 points per problem, 12 points total) Atoms a. 3.4 x 1026 atoms C. 9.0 x 1020 atoms Moles 0.1250 moles b. 0.0015 moles d.

What is a cultural trait? OA OB. O C. OD. a behavior common to all cultures an element of culture that depends on people an element of culture that is adopted from other cultures a behavior unique to a cultural group

Write the correct chemical formula on the blanks: • Potassium bicarbonate . Carbon tetrafluoride . . . Nickel II Oxide Aluminum Hydroxide Hydrogen Fluoride . Nickel III Oxide . • Silicon dioxide . . Sulfur hexafluoride Dinitrogen monoxide Cobalt II Chloride I • CoCl₂ • FeSO4 • Mg(OH)2 . CF4 • SiO2 • N₂O • Ni2O3 • HNO3 • FeS • AICI3 • NiO • SF6 • H2SO4 。 Al(OH)3 (5 points) • HF • KHCO3 • CoCl3

Compound Mass Moles H₂O N₂O SO₂ CH₂Cl₂ 113 6.11 g 2.72 0.0784 Number of molecules Complete the fourth column of the table.. Enter your answers numerically separated by commas. Nho, NN₂0 Nso₂ NCH₂Cl₂ Submit VAXO ? 45.34 1026,0.837 1023, 16.379 1023, 0.67211023 Previous Answers Request Answer

Using the two tables below and your knowledge of the shapes of molecules, identify whether each of the compounds below are polar or nonpolar by writing polar or nonpolar next to the compound. (3 points per compound 9 points total) a. b. C. SeO₂ NBr3 CO₂

13. For the following equations and the number of grams of starting materials given, determine the limiting reactant and the number of grams of the designated product actually produced. 20 points) 2 Na3PO4 + 3 MgCl2 →Mg3(PO4)2 + 6 NaCl starting materials 250. grams MgCl2 and Limiting reactant = Grams of Mg3(PO4)2 200. grams Na3PO4

Combine the following pairs of reactants in test tubes by using the stock solutions in the lab. Use about 1-2 mL of each solution. Describe each reaction. (NH4)2CO3(aq) + CaCl₂(aq) (NH4)2CO3(aq) + K₂SO4(aq) Ba(NO3)2(aq) + CaCl₂(aq) Ba(NO3)2(aq) + K₂SO4(aq) -> You will be using a glass pipette and a pipette bulb. Do not invert or turn the pipette sideway or the chemical inthe pipet will touch the pipet bulb. And when you reuse the pipet bulb, you contaminate all chemical. (watch video 7 on the first page please) FAJORT 1 1 Lab Report Write balanced molecular equations and balanced net ionic equations for the four reactions. Include designations for state of matter, e.g. (aq) and (s). Write N.R. if no reaction occurred.

Which of the following exists as separate ions and should thus be split up in a net-ionic equation? (Choose all that should be split and be aware of the state) O₂(aq) HCI(g) KBr(aq) ✔aqueous ethanol - CH₂CH₂OH(aq) NaCl(s) HF(aq)

An unknown metal absorbs 23.8 J of heat, and its temperature increases by 15.4°C. What is the heat capacity of the metal? • Round your answer to two decimal places. Provide your answer below: J/degrees C FEEDBACK

Select the single best answer. Arrange the compounds NaF, MgO, and AIN in order of increasing lattice energy. MgO, AIN, NaF MgO, NaF, AIN NaF, AIN, MgO NaF, MgO, AIN AIN, MgO, NaF AIN, NaF, MgO

Ammonium nitrate (NH4NO3) dissolves readily in water eventhough the dissolution is endothermic by 26.4kj/mol. The solution process is spontaneous because 1. of the increase in enthalpy upon dissolution of this strong electrolyte 2. the vapor pressure of the water decreases upon addition of the solute 3. of the increase in disorder upon dissolution of this strong electrolyte 4. osmotic properties predict this behavior 5. of the decrease in enthalpy upon addition of the solute

A chemist must dilute 64.0 mL of 2.29 M aqueous sodium carbonate (Na₂CO3) solution until the concentration falls to 2.00 M. She'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Round your answer to 3 significant digits.

How many moles of NH3 can be produced from 3.04 moles of nitrogen in the following reaction: N₂ (g) + 3 H₂ (g) → 2 NH3 (g)

Calculate the mass (in grams) of CO2 produced by the reaction of 0.130 mol of HCl with excess NaHCO3. Do not include units in your answer. HCI (aq) + NaHCO3(aq) → NaCl (aq) + H₂O () + CO₂(g) Answer:

When solutions of lead(II) nitrate and sodium sulfate are mixed, a white precipitate forms. Write the balanced chemical equation for this reaction. Phases are optional. Do not write an ionic equation (i.e., the answer should not show any charges).

Part A For the reaction, calculate how many moles of the product form when 1.83 mol of H₂ completely reacts. Assume that there is more than enough of the other reactant. H₂ (g) + Cl₂ (g) → 2 HCl (g) VHCI = Part B For the reaction, calculate how many moles of the product form when 1.95 mol of O2 completely reacts. Assume that there is more than enough of the other reactant. 2 H₂ (g) + O2 (g) → 2 H₂O (1) VH2O=

The rust that appears on steel surfaces is iron(III) oxide. If the rust found spread over the surfaces of a steel boat hull contains, a total of 1.324 x 1023 oxygen atoms, how many grams of rust are present on the boat hull? mass:

A double bond between two atoms, A and B, _______________. arises when two electrons are transferred from A to B. is longer than a single bond between the same two atoms. has a lower bond energy than a single bond between the same two atoms. consists of four electrons shared between A and B. consists of two electrons shared between A and B.

Give the chemical symbol for the element with the ground-state electron configuration [Ar]4s²3d². symbol: Determine the quantum numbers n and and select all possible values for me for each subshell of the element. 4s n = 4s = The possible values of me for the 4s subshell are 0 -3,-2,-1,0, +1, +2, +3 -2,-1,0, +1, +2 -1,0, +1

Upon mixing a clear colorless BaCl 2 solution with a clear, colorless Na 2SO 4 solution according to the reaction below, a student observes a white cloudiness form. What is responsible for the cloudiness that is observed? BaCl 2(aq) + Na 2SO 4(aq) → BaSO 4(s) + 2NaCl(aq) Na2SO4 NaCl BaCl2 BaSO4 It is impossible to tell without doing the reaction oneself.

What is the most likely cause of a large Portuguese-speaking population in Brazil? A. Brazil is surrounded by Spanish-speaking countries. B. Portugal and Brazil have developed good trade relations. C. Portugal had established a colony in Brazil in the past. D. Portugal and Brazil have engaged in wars in the past.

Write the balanced net ionic equation for the reactions that occur when the given aqueous solutions are mixed. Include the physical states. A. nitric acid, HNO3, and calcium hydroxide, Ca(OH)2 net ionic equation: B. lead(II) nitrate, Pb(NO3)2, and potassium iodide, KI net ionic equation:

MnO₂ (s) + HCl(aq) → Cl₂ (g) + MnCl₂ (aq) + H₂O(1) Express your answer as a chemical equation. Identify all of the phases in your answer. A chemical reaction does not occur for this question. Part B CO2 (g) +BaSiO3 (s) + H₂O(1)→ SiO2 (s) + Ba(HCO3)2 (aq) Express your answer as a chemical equation. Identify all of the phases in your answer.

Assuming reactions between the following pairs of elements, which pair is most likely to form an ionic compound? fluorine and iodine chlorine and oxygen copper and tin carbon and chlorine cesium and iodine

Be sure to answer all parts. Rank the following compounds in order of increasing strength of intermolecular forces: A. CH3CH₂CH₂CHO (butanal) B. CH3CH₂CH₂CH₂CH3 (pentane) C. CH3CH₂CH₂CH₂OH (1-butanol)

A gas occupies a volume of 25.0 mL at a pressure of 760.0 mmHg and 27.0°C. What is the volume of the gas when the pressure is changed to 500.0 mmHg and the temperature to 400 K? 760 mm Hg = 1 atm.

Fe(NO3)3(aq) + (NH4)2S (aq) → Fe2 S3 (s) + NH4NO3(aq) Express your answer as a chemical equation. Identify all of the phases in your answer.

Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce ammonia. N₂(g) + 3 H₂(g) → 2 NH3(g) Assume 0.280 mol N₂ and 0.901 mol H₂ are present initially. After complete reaction, how many moles of ammonia are produced? NH3: mol How many moles of H₂ remain? H₂: mol

Gaseous hydrogen and oxygen can be prepared in the laboratory from the decomposition of gaseous water. The equation for the reaction is 2 H₂O(g) →2H₂(g) + O₂(g) Calculate how many grams of O₂(g) can be produced from 66.8 g H₂O(g). mass: g 0₂

For the reaction shown, calculate how many moles of NO₂ form when each amount of reactant completely reacts. 2 N₂O5 (g) →4 NO2 (g) + O2(g) Part D 1.009 x 10-³ mol N₂O5 Express your answer using four significant figures.

Write the new moles ratios for the following equations based on the information given 1. 2Na+ O₂ → Na₂O using 3 moles O₂ 2. Pb(NO3)2 + 2KIPbl2 + 2KNO3 starting with 4 moles KI 3. 2Al + 3CuCl₂ ⇒ 2AlCl3 + 3Cu starting with 0.05 moles CuCl2 4.2H₂O → 2H₂ + O₂ making 760 moles of H₂. 5. CH4 + 202 CO2 + 2H₂O making 51 moles H₂O

Consider the following reaction at equilibrium: 2NO₂(g) ⇒ N₂O4(g) The AH' for this reaction is <0. If the volume of the container is decreased by while the temperature is kept constant, how will K(eq) change? A) increase B) decrease C) stay the same

List the number of each type of atom on the right side of the equation 2 Na3PO4 (aq) + 2 CoCl₂ (aq) → 2C03 (PO4)2 (s) + 6NaCl(aq) Enter your answers separated by commas (the order of the numbers is the same as the order of the elements on the left side of the equation).

Which statement best describes the process of Alpha and Beta Decay? (Pick 2) In Alpha Decay the atom gains 2 protons and 2 neutrons. In Alpha Decay the atom loses 2 protons and 2 neutrons. In Beta Decay one of the atoms neutrons splits into a proton and electron. In Beta Decay one of the atoms protons and electrons combine to form a neutron.

List the number of each type of atom on the left side of the equation C2H6 (g) + 7 O2 (g) → 3 CO2 (g) + 6 H₂O(g) Enter your answers separated by commas (the order of the numbers is the sam order of the elements on the left side of the equation). Part E List the number of each type of atom on the right side of the equation C2H6 (g) + 7O2(g) → 3CO2 (g) + 6H₂O(g) Enter your answers separated by commas (the order of the numbers is the same as order of the elements on the left side of the equation).

Which of the following molecules are aliphatic hydrocarbons? CH3CH3 CH3CH₂OH CH2=CH₂ I Multiple Choice I and III I, II, III II II and IV II, III, IV III CH3OCH3 IV

As the separation distance between two charges of the same sign increases, what happens to the electrostatic potential energy? It becomes more negative (i.e., lower) It becomes less positive (i.e., lower) It becomes more positive (i.e., higher) It becomes less negative (i.e., higher)

The indicated carbon atom is: -Br Multiple Choice O O O Electrophilic because it is electron-rich. Nucleophilic because it is electron-deficient. Nucleophilic because it is electron-rich. Electrophilic because it is electron-deficient.

How many molecules of water are made from the reaction of 35 moles of HCl with excess oxygen? Given the reaction: 4 HCl + O₂ → 2 H₂O + 2Cl₂ O 5.3 x 1024 O 2.1 x 1024 O 4.2 x 1025 O 3.8 x 1024 5.8 x 10-23 2.9 x 10-23 O 1.1x 1025

Which atomic orbitals overlap to form the carbon-carbon σ and TT bonding molecular orbitals of ethylene, H₂C=CH2? Multiple Choice O O O Csp³ + Csp³, and C2p+C2p Csp³ + Csp³, and Csp² +Csp² Csp²+Csp², and Csp²+ Csp² Csp²+Csp², and C2p+C2p

Return to the balanced equation O₂ 1-2 H₂ → 2H₂O (1pts) 16. a. How many moles are in 39 grams of O₂? (1pts) b. Using the calculated moles of O₂ from 16a, how many moles of H₂O can you make? (1pts) c. Using the calculated moles of H₂O from 16b, how many grams of H₂O can you make? Now we will use the chemical equation N₂ + 3 H, -> 2NH, (1pts) 17. If you begin with 18.3 grams of N₂, how many grams of NH3 can you make?

One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose an EPA chemist tests a 250. mL sample of groundwater known to be contaminated with tin(II) chloride, which would react with silver nitrate solution like this: SnCl₂(aq) + 2 AgNO3(aq) - mg 2 AgCl(s) + Sn(NO3)₂(aq) The chemist adds 32.0 mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 8.2 mg of silver chloride. Calculate the concentration of tin(II) chloride contaminant in the original groundwater sample. Round your answer to 2 significant digits.

Calculate the solubility at 25 °C of CaF2 in pure water and in a 0.0170 M NaF solution. You'll find Ksp Round both of your answers to 2 significant digits. data in the ALEKS Data tab.

O Resonance structures have the same placement of electrons but different arrangement of atoms. Resonance structures have the same placement of atoms but different arrangement of electrons. Resonance structures have the same placement of atoms and the same arrangement of electrons. Resonance structures have different placement of atoms and different arrangement of electrons.