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Exam 13: Chemical Kinetics Clearing the Air

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Question 31

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A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step 1: H₂(g) + 2 NO(g) $\rightarrow$ N₂O(g) F+H₂O(g) (slow) Step 2: N₂O(g) +H₂(g) $\rightarrow$ N₂(g) +H₂O(g) (fast) What is the rate law for step 1?

A) k[H₂][NO]
B) k[H₂][NO]²
C) k[H₂]²[NO]
D) k[H₂]²[NO]²
E) More information is needed.

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Question 32

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The energy profiles for four different reactions are shown.Which of the reactions will have the largest rate constant?

A) A
B) B
C) C
D) D
E) More information is required.

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Question 33

Multiple Choice

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Which statement below regarding catalytic converters is FALSE?

The following figure shows Arrhenius plots for four different reactions.Which reaction has the lowest frequency factor?

The mechanism for the reaction 2 H₂O₂ (aq) $\rightarrow$ 2 H₂O(l) + O₂(g) in the presence of I^-(aq) is proposed to be: Step 1: H₂O₂(aq) + I^-(aq) $\rightarrow$ H₂O(l) + OI^-(aq) (slow) Step 2: H₂O₂(aq) + OI^-(aq) $\rightarrow$ H₂O(l) + O₂(g) +I^-(aq) (fast) What is the rate law for the overall reaction?

The reaction A + 2B $\rightarrow$ C is first order in B and A.The overall order of the reaction is

For the second-order reaction $\mathrm{NO}(g)+\mathrm{F}_{2}(g) \rightarrow \mathrm{NOF}(g)+\mathrm{F}(g)$ the value of the rate constant increases from 4.72 *10⁷ M ^-1s^-1 at 298 K to 1.21* 10⁸ M^-1s^-1 at 473 K.Estimate the activation energy of the reaction.

For the reaction 3A + 2B $\rightarrow$ 5C + 4 D, the rate of the reaction in terms of $\Delta$ [A]/ $\Delta$ t would be written as _______ .

The linear form of _______ is very useful, as it allows us to calculate the activation energy and the frequency factor.

The rate of a reaction is found to increase nine-fold when the concentration of one reactant is tripled. The order of the reaction with respect to this reactant is

The energy profiles for four different reactions are shown.Which of the reactions will have the smallest rate constant?

For the rate law Rate =k[A]^1/2[B], the partial order with respect to A is _______ , the partial order with respect to B is _______ , and the total order is _______ .

A scientist conducts an experiment to determine the rate of the following reaction: 2 N₂(g) +O₂(g) $\rightarrow$ 2 N₂O(g) If the initial concentration of N₂ was 0.400 M and the concentration of N₂ was 0.350 M after 0.100 s, what is the average rate of reaction over the first 100 milliseconds?

The linear form of the Arrhenius equation is very useful as a plot of _______ , as it allows us to calculate the activation energy and the frequency factor.

The observed rate law for the reaction H₂ (g) + 2 ICl(g) $\rightarrow$ I ₂ (g) + 2 HCl(g) is first order with respect to each reactant.Draw an energy diagram that shows energy versus reaction progress for the mechanism given.Both steps are exothermic.

For the first-order reaction 2 SO₂ Cl(g) $\rightarrow$ 2 SO₂ (g) +CL₂ (g) , it takes 3.50 minutes for the concentration of SO₂Cl to decrease from 0.250 M to 0.205 M when the temperature is 25.0 $\degree$ C.How long will it take for the reaction to be 75.0% complete?

Which reaction below is NOT important in the production of photochemical smog?

Which of these could be the units for the rate constant in a second-order reaction?

A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step 1: H₂(g) + 2 NO(g) $\rightarrow$ N₂O(g) +H₂O(g) (slow) Step 2: N₂O(g) + H₂(g) $\rightarrow$ N₂(g) +H₂O(g) (fast) Which of the following statements is NOT true?

The rate at which gas-phase hydrogen and iodine react to form hydrogen iodide, H₂(g) +I₂(g) $\rightarrow$ 2 HI(g), can be increased by using a platinum catalyst.Suppose the uncatalyzed reaction has an activation energy of about 180 kJ while that of the catalyzed reaction is about 60 kJ at 600 K.Approximately how many times faster is the catalyzed reaction relative to the uncatalyzed? Assume the frequency factor is the same for both processes.