S pts) For the folwngquestionsosider the following reaction mechanism I A Step 1
ID: 1030018 • Letter: S
Question
S pts) For the folwngquestionsosider the following reaction mechanism I A Step 1 Step 2 Step 3 fast fast slow (a) Which step(s) is the rate-limiting step? (2 pts) Explain (2 pts) (b) Which species are reaction intermediates? (2 pts) Which species might be the catalyst? (2 pts) 36. (6 pts) Consider the reaction At equilibrium, [CO]-3.5 x 10 M: [Cl,]-4.1x10 M, and [COCI,]-0.068 M. Calculate the value of the equilibrium constant, K 2.1x IO cC, the value of the equilibrium constant Kis 1.2x 10. What 37. (8 pts) For the chemical equilibrium aA +bB is the value of the equilibrium constant for the reaction 3 cC 3 aA+3 bB?Explanation / Answer
35a) Step 3 is the rate-limiting step of the reaction. This is due to the fact that step 3 is the slowest step of the reaction. Steps 1 and 2 occur fast to produce the intermediate or the product. However, the reaction is not complete unless step 3 occurs. Step 3 occurs slowly and hence, the rate of the reaction is governed by the rate at which step 3 occurs.
b) A reaction intermediate is a species which is generated in one particular step of the reaction and consumed in another. The intermediate doesn’t appear at the end of the reaction. From the given mechanism, it is clear that Z and V are the intermediates. Z is produced in step 1 of the reaction and consumed in steps 2 and 3. Similarly, V is produced in step 2 of the reaction and consumed in step 3.
A catalyst is a species that accelerates the reaction without itself undergoing any change in the reaction. The catalyst participates in one or more steps of the reaction, but is re-generated at the end of the reaction. Clearly Y is used in step 1 and is regenerated in the step 3 of the reaction. Hence, Y is the catalyst.
37) The equilibrium constant expression for the reaction is
K = [C]c/[A]a[B]b = 1.2*103
Write down the equilibrium constant expression for the reaction asked in question as
K’ = [A]3a[B]3b/[C]3c = {[A]a[B]b/[C]c}3 = (1/K)3 = 1/K3 = 1/(1.2*103)3 = 5.78*10-10 (ans).
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