Part II Multiple Choice. Circle the selection that best answers each question. 1

Question

Part II Multiple Choice. Circle the selection that best answers each question. 1. For the reaction: 10, (aq)+ST (ag)+ 6H'(ag) 31-(ag)+3H O0) the rate of disappearance of I-(a) at a particular time and concentration is 2.6 x 10 mol/(L s). What is the rate of appearance of (ag)? a. 4.3 x 103 mol/(L s) b. 7.8x 10-3 mol(L s) c. -1.6x 103 mol/(L s) d. 1.6x 103 mol/(L s) e. 6.4x 10 3 mol/(L-s) 2. In a chemical reaction at constant temperature, the addition of a catalyst. provides an alternative reaction pathway with a different activation energy a. b. increases the concentration of the products at equilibrium. c. affects the equilibrium constant. d. increases the fraction of molecules with more than a given kinetic energy e. decreases the energy released in the chemical reaction. 3. One mechanism for the depletion of ozone in the stratosphere is proposed as follows: (1) CI+O CIO+ O2 (2) CIO +O-CI+O Identify any catalysts and intermediates in the reaction. a. Cl is a catalyst, there are no intermediates. b, O is an intermediate, CIO is a catalyst. c. O2 is a catalyst, O is an intermediate. d. CIO is a catalyst, there are no intermediates. e. Cl is a catalyst, CIO is an intermediate. 4. If a reaction is second-order in a reactant, when the concentration of the reactant is increased by a factor of 2, the reaction rate will a. Remain constant. b. Increase by a factor of 2 c. increase by a factor of 4. d. increase by a factor of 6. e. increase by a factor of 8. 5. Select the molecule with the highest boiling point. a. CHCb b. Cl 6. Which of the following aqueous solutions would have the highest boiling point? c. CHCH20H d. Fe(OH)2 e. H2O 7. Which of the following can we predict from an equilibrium constant for a reaction? (1) The extent of a reaction (2) Whether the reaction is fast or slow (3) Whether the reaction is exothermic or endothermic b. 3 only c. 3 only d.1 and 2 e. 1 and 3 a. 1 only

Explanation / Answer

1)

rate of reaction = (1/5)*rate of disappearance of I-

similarly:

rate of reaction = (1/3)*rate of appearance of I2

equating both:

(1/3)*rate of appearance of I2 = (1/5)*rate of disappearance of I-

rate of appearance of I2 = (3/5)*rate of disappearance of I-

= (3/5)*(2.6*10^-3 mol/L.s)

= 1.6*10^-3 mol/L.s

Answer: d

2)

Adding catalyst provide other pathway with lower activation energy

Answer: a

Only 1 question at a time please

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