1. (10 points) Consider the following reaction: CH3Br(a) +OH-(aq) -> CH3OH(aq) +
ID: 706675 • Letter: 1
Question
1. (10 points) Consider the following reaction: CH3Br(a) +OH-(aq) -> CH3OH(aq) + Br(aq) The rate law for this reaction is first order in CH3Br and first order in OH-. When [CH3Brl is 0.050 M and [OH-] is 0.105 M, the reaction rate at 298 K is 0.16 M/s. What is the value of the rate constant? 2. (10 points) The reaction 2 NO(g) + Cl2(g) ? 2 NOCl(g) has had the following mechanism proposed: NO(g)+ Cl2(g) ? NOC12(g) NOCI2g)+ NO() - 2 NOCI(g) If the first step is much slower than the second step, what should be the rate law?Explanation / Answer
Ans 1 :
The rate law expression is given as :
Rate = k{CH3Br] [OH-]
Putting all the values :
0.16 = k (0.050) (0.105)
k = 30.476 M-1s-1
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