Review Materials in General Chemistry 2 (Second Semester)

D

Study the picture BELOW. Which of the following CORRECTLY predicts the entropy change and its spontaneity?

A. ΔS = +ve and nonspontaneous

B. ΔS = -ve and spontaneous

C. ΔS = -ve and nonspontaneous

D. ΔS = +ve and spontaneous

D

Study the picture BELOW. What statement BEST explains the Second Law of Thermodynamics?

A. If the physical process is reversible, the combined entropy of the system and the environment must decrease.

B. If the physical process is reversible, the combined entropy of the system and the environment must increase.

C. If the physical process is irreversible, the combined entropy of the system and the environment must decrease.

D. If the physical process is irreversible, the combined entropy of the system and the environment must increase.

A

Study the picture BELOW. Entropy increases from solid, liquid to gas. Why?

A. Because molecular disorder increases

B. Because molecular randomness decreases

C. Because molecules are more energetic

D. Because molecules are more reactive

A

Look at and study the picture BELOW. Gibbs free energy change is equal to

A. ∆H - T∆S

B. ∆H - S∆T

C. ∆G - T∆S

D. ∆H + T∆S

A

Study the picture BELOW. Consider a process for which ΔH = 211 kJ and ΔS = -57 J/K. How will raising the temperature affect ΔG for this process?

A. ΔG will increase.

B. ΔG will decrease.

C. ΔG will not change.

D. The effect on ΔG cannot be predicted from the information given

B

Study the diagram BELOW. Which statement is NOT TRUE about the chemical equilibrium in terms of the reaction rates of the forward and the reverse reaction?

A. The amounts of the reactants and products are observed to be constant after some time.

B. The rate of the product formed from the reactant is NOT equal to the rate of the reverse reaction.

C. The rate of the product formed from the reactant is equal to the rate of the reverse reaction.

D. The chemical equilibrium is derived from the formula; [R] = K1; [P] = K1 x K2.

A

Which of the following statements BEST explains the three (3) substances in terms of their chemical equilibrium?

A. (a) Initially, the concentration of SO3 is twice as much as that of SO2. At equilibrium, a mixture of all three gases is obtained. (b) Initially, only SO2 is present.

B. (a) Initially, the concentration of SO2 is twice as much as that of SO3. At equilibrium, a mixture of all three gases is obtained. (b) Initially, only O2 is present.

C. (a) Initially, the concentration of SO2 is twice as much as that of O2. At equilibrium, a mixture of all three gases is obtained. (b) Initially, only SO3 is present.

D. (a) Initially, the concentration of O2 is twice as much as that of SO2. At equilibrium, a mixture of all three gases is obtained. (b) Initially, only SO3 is present.

D

Study the pictures BELOW. Given N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g), which scenario will allow you to eventually reach an equilibrium mixture involving these chemicals?

A. Place only N2 into a sealed vessel.

B. Place only H2 into a sealed vessel.

C. Place only NH3 into a sealed vessel.

D. Place N2 and NH3 into a sealed vessel.

C

Study the pictures BELOW. Given the reaction CO(g) + 3H2(g) ⇌ CH4 + H2O(g) at the equilibrium concentration [CO] = 4.0 M; [H2] = 2.8 M; [CH4] = 0.75 M; and [H2O] = 0.12 M, what is the equilibrium constant (Keq)? (Round off your answer to the correct number of significant figures.)

A. Keq = 1.6 x 104

B. Keq = 6.5 x 10-6

C. Keq = 1.5 x 10-5

D. Keq = 3.2 x105

B

Study the picture BELOW. Which of the following statements CORRECTLY states the Le Chatelier’s Principle?

A. It states if a chemical system at equilibrium is stressed, the system will adjust to increase the stress.

B. It states if a chemical system at equilibrium is stressed, the system will adjust to reduce the stress.

C. It states if a chemical system at equilibrium is stressed, the system will not adjust.

D. It states if a chemical system at equilibrium is stressed, the system will adjust.

A

Study the pictures BELOW. In the reaction, CO (g) + NO2 (g) ↔ CO2 (g) + NO (g), which of the following changes would result in the formation of more products at equilibrium?

A. Increasing the pressure

B. Removing CO (g) from the reaction

C. Adding NO2 (g) to the reaction

D. Adding CO2 to the reaction.

C

Study the picture BELOW. Which statement describes the Brønsted – Lowry acid and Brønsted – Lowry base?

A. An acid is a proton donor, and a base is an electron donor.

B. An acid is a proton acceptor, and a base is an electron acceptor.

C. An acid is a proton donor, and a base is an electron acceptor.

D. An acid is a proton acceptor, and a base is an electron donor.

A

Study the pictures BELOW. In the reaction, CO (g) + NO2 (g) ↔ CO2 (g) + NO (g), which of the following changes would result in the formation of more products at equilibrium?

A. Increasing the pressure

B. Removing CO (g) from the reaction

C. Adding NO2 (g) to the reaction

D. Adding CO2 to the rection

C

Study the picture BELOW. Which statement describes the Brønsted – Lowry acid and Brønsted – Lowry base?

A. An acid is a proton donor, and a base is an electron donor.

B. An acid is a proton acceptor, and a base is an electron acceptor

C. An acid is a proton donor, and a base is an electron acceptor.

D. An acid is a proton acceptor, and a base is an electron donor.

D

Study the picture BELOW. What might happen if you mixed a strong acid with an equally sturdy base?

A. You would see an explosive chemical reaction.

B. The acid would destroy the base.

C. The base would destroy the acid.

D. You would wind up with a pH-neutral substance.

B

Study the picture BELOW. Which of the following statements is TRUE concerning acid-base properties in water?

A. Acid and base do not react with each other.

B. Acid mixed with base neutralizes each other.

C. Acid mixed with base makes a sturdy base.

D. Acid mixed with base makes a weak base.

A

Study the picture BELOW. Which of the following statements BEST states the autoionization of water?

A. The process where water can combine with itself acting as both an acid and a base

B. The process where water can act like an acid donating hydrogen ions

C. The process where water can combine with stronger chemicals

D. The process where water can form hydrogen bonds in solution

A

Study the picture BELOW. The [OH -] of a certain base is 2.9 x 10-4 M. Calculate the pH (power of hydrogen) of the solution. (Round off your answer to the correct number of significant figures.)

A. pH = 10.

B. pH = 10.4

C. pH = 10.46

D. pH = 10.464

C

Study the picture BELOW. Which solution has the higher pH?

A. A 0.1 M solution of an acid with Ka = 1 X 10-4 or one with Ka = 4 X 10-5

B. A 0.1 M solution of an acid with pKa = 3.0 or one with pKa = 3.5

C. A 0.1 M solution of a weak acid or a 0.01 M solution of the same acid

D. A 0.1 M solution of a weak acid or a 0.1 M solution of a strong acid

B

Study the picture BELOW. What is the pH of 0.0111 M NaOH? Is the soln neutral, acidic, or basic? (Round off your answer to the correct number of significant figures.)

A. 12.2; acidic

B. 12. 1; basic

C. 12. 3; neutral

D. 12. 5; basic

C

Study the picture BELOW. Which of the following statements is TRUE about buffer solution?

I. pH of buffer solution will never change despite addition of small amount of base or acid.

II. Buffer can be made by mixing weak acid and salt of its conjugate base or by mixing weak base with salt of its conjugate acid.

III. Buffer has acid and base components that can work specifically to resist pH change.

IV. The closer the ratio of concentration weak acid/base to the concentration of salt of its conjugate base/acid, the less effective the buffer to resist pH change.

A. I

B. IV

C. II and III

D. I and IV

D

Study the pictures BELOW. A buffer soln is prepared from 0.24 M NH3 and 0.20 M NH4Cl. What is the pH of this buffer? (Round off your answer to the correct number of significant figures.)

A. pH = 9. 53

B. pH = 9. 35

C. pH = 9. 43

D. pH = 9. 34

B

Study the picture BELOW. The terms Oxidation and Reduction have direct opposite definitions. What is each term defined as?

A. Oxidation – something having to do with oxide, I do not care -, Reduction – something is being reduced, but I do not know what.

B. Oxidation – the loss of electrons by atom or ion / the gain of oxygen, Reduction – the loss of oxygen / the gain of said electrons.

C. Oxidation – the gain of electrons by an atom or ion/loss of oxygen, Reduction – the gain of oxygen / the loss of electrons by atom or ion.

D. Oxidation - the loss of protons by atom or ion / the gain of oxygen, Reduction – the loss of oxygen / the gain of said protons

A

Study the pictures BELOW. In the reaction Zn + H2O --> ZnO + H2, which element, if any, is oxidized?

A. Zinc

B. Hydrogen

C. Oxygen

D. None of the above

A

Based on the pictures BELOW, what substance is the reducing agent in the following reaction?

4Fe + 3O2 --> 2Fe2O3

A. Iron

B. Fluorine

C. Oxygen

D. Hydrogen

B

Study the pictures BELOW. Consider the reaction: Ag+(aq) + Zn(s) → Ag(s) + Zn(2+)(aq). Which equation has a CORRECT balanced redox reaction using oxidation number method?

A. 3Ag+(aq) + Zn(s) → 3Ag(s) + Zn2+(aq)

B. 2Ag+(aq) + Zn(s) → 2Ag(s) + Zn2+(aq)

C. Ag+(aq) + Zn(s) → Ag(s) + Zn2+(aq)

D. 4Ag+(aq) + Zn(s) → 4Ag(s) + Zn2+(aq)

D

Study the pictures BELOW. Using the oxidation number method, what equation has a CORRECT balanced redox reaction?

Cu(s) + HNO3(aq) → Cu (NO3)2(aq) + NO2(g) + H2O(l)

A. Cu(s) + 3HNO3(aq) → Cu (NO3)2(aq) + 3NO2(g) + 3H2O(l)

B. Cu(s) + 5HNO3(aq) → Cu (NO3)2(aq) + 4NO2(g) + 6H2O(l)

C. Cu(s) + 2HNO3(aq) → Cu (NO3)2(aq) + 5NO2(g) + 4H2O(l)

D. Cu(s) + 4HNO3(aq) → Cu (NO3)2(aq) + 2NO2(g) + 2H2O(l)

A

Study the pictures BELOW. Which of the following equations has a CORRECT balanced redox reaction?

K2Cr2O7(aq) + HI (aq) → KI (aq) + CrI3(aq) + I2(s) + H2O

A. 2K2Cr2O7(aq) + 14HI (aq) → 2KI (aq) + 2CrI3(aq) + 3I2(s) + 7

B. K2Cr2O7(aq) + 10HI (aq) → 3KI (aq) + 6CrI3(aq) + 3I2(s) + 74H2O(l)

C. K2Cr2O7(aq) + 14HI (aq) → 2KI (aq) + 2CrI3(aq) + 3I2(s) + 7H2O(l)

D. 4K2Cr2O7(aq) + 14HI (aq) → 4KI (aq) + 4CrI3(aq) + 3I2(s) + 7H2O(l)

D

Study the picture BELOW. In an electrolytic cell the electrode at which the electrons enter the solution is called the ______; the chemical change that occurs at this electrode is called _______.

A. anode, oxidation

B. anode, reduction

C. cathode, oxidation

D. cathode, reduction

C

Study the picture BELOW. Which potential of an electrochemical cell can be computed as the difference between the standard reduction electrode potentials of the cathode and the anode?

A. Reduction

B. Oxidation

C. Cell

D. Tissue

B

Study the picture BELOW. Given their standard reduction potential, which of the species is going to be oxidized?

Cu2+/Cu = 0.34V

Zn2+/Zn = -0.76V

A. Cu

B. Zn

C. CuSO4

D. ZnSO4

C

Study the pictures BELOW. Consider the galvanic cell given. Which of the following deductions about this cell is CORRECT?

A. Oxidation is occurring in half-cell 2.

B. The positive electrode is in half-cell 2.

C. Oxidation is occurring in half-cell 1.

D. The negative electrode is in half-cell 1.

D

Study the picture BELOW. The standard cell potential for the cell or cell emf, Mg(s), / Mg2+ (1 M, aq) // Sn2+ (1 M, aq) / Sn(s) is:

(Round off your answer to the correct number of significant figures.)

Mg2+ + 2e- → Mg E° = -2.36 V

Sn2+ + 2e- → Sn E° = -0.14 V

A. -2.20 V

B. +2.20 V

C. -2.50 V

D. +2.50 V

D

Given that the standard reduction potential of Zn2+ is -0.76 V, calculate the E°red for the reduction of Cu2+ to Cu. (Round off your answer to the correct number of significant figures.)

Cu2+(aq, 1 M) + 2e- → Cu(s)

A. 0.35 V

B. 0.36 V

C. 0.33 V

D. 0.34 V

D

The standard emf for this cell is 1.46 V. Using the data in the Table 20.1 below, what is the E°red for the reduction of In3+ to In+? (Round off your answer to the correct number of significant figures.)

A. -0.401 V

B. -0.402 V

C. -0.403 V

D. -0.400 V

D

Study the picture BELOW. Which of the following statements is NOT TRUE about an electrochemical cell?

A. An electrochemical cell produces electricity.

B. The flow of electrons in an electrochemical cell is from the anode to the cathode.

C. The salt bridge of an electrochemical cell allows the transfer of charges in the form of electrons.

D. The electrochemical cell requires no energy input.

A

Study the picture BELOW. What happens to the cell voltage when the salt bridge is removed?

A. The cell voltage drops to zero.

B. The cell voltage increases.

C. The cell voltage becomes negative.

D. The cell voltage is anged.

C

Below shows a cell diagram for voltaic cell. Which of the following is FALSE?

A. Electrons flow from anode to cathode.

B. Oxidation happens in the anode.

C. Copper undergoes reduction to form copper ion.

D. Zinc undergoes oxidation to form zinc ion

A

Study the picture BELOW. In the case of a lead-acid battery, during discharging

A. both anode and cathode become PbSO4.

B. specific gravity of acid increases.

C. voltage of the cells increases.

D. only anode produces electricity.

C

Study the picture BELOW. Imelda wants to make her ring more beautiful. She also wants to prevent it from corrosion. What is the BEST way she must do?

A. Dip the ring in oil.

B. Wash the ring with soap.

C. Plate the ring with gold.

D. Polish the ring with water

A

Study the picture BELOW. Which statement does NOT explain inert electrodes?

A. They do not react with the compounds undergoing redox reactions.

B. They are necessary only for gases and aqueous solutions.

C. They function as the site for redox reactions.

D. They can be used as metallic electrodes.

A

An experiment is set up as shown in the diagram BELOW. Both electrodes P and Q are made of graphite. Which of the following gives the CORRECT results as electrolysis proceeds?

A. Electrolytes: Aqueous sodium chloride; Mass of P: Stays unchanged; Mass of Q: Increase

B. Electrolytes: Aqueous sodium chloride; Mass of P: Increase; Mass of Q: Remains unchanged

C. Electrolytes: Aqueous copper (II) sulfate; Mass of P: Stays unchanged; Mass of Q: Increase

D. Electrolytes: Aqueous copper (II) sulfate; Mass of P: Increase; Mass of Q: Stays unchanged

B

What is the material used to make inert electrode?

A. Copper

B. Aluminum / Aluminium

C. Zinc

D. Mercury

D

Platinum electrode is ______ electrode while iron electrode is ______ electrode.

A. active electrode, active electrode

B. active electrode, inert electrode

C. inert electrode, inert electrode

D. inert electrode, active electrode

C

Study the picture BELOW. If a nail is placed in salt water, what will MOST LIKELY happen to it?

A. It will oxidize.

B. It will reduce.

C. It will rust.

D. It will electrolyze.

D

Study the picture BELOW. If a nail is placed in dry air with anhydrous calcium chloride, what do you think will happen to it?

A. It will not reduce.

B. It will not oxidize.

C. It will not electrolyze.

D. It will not rust

B

Study the picture BELOW. If the spoon is to be electroplated with silver metal, what electrolyte should be used?

A. Molten silver chloride

B. Aqueous silver nitrate

C. Sodium chloride solution

D. Copper (II) sulfate solution