1. The reaction A + 2B C is zero order in A & first order in B. The rate is 0.01

ID: 886701 • Letter: 1

Question

1. The reaction A + 2B C is zero order in A & first order in B. The rate is 0.012 mol L-1 s-1

when [A] is 0.020 and [B] is 0.60 M. Determine k (include units) and find the reaction rate

when A and B are each 0.010 M.

2. For the following reaction of hexacarbonyl molybdenum,

Mo(CO)6 + P(CH3)3 Mo(CO)5P(CH3)3 + CO

the proposed mechanism is

Step 1: Mo(CO)6 Mo(CO)5 + CO

Step 2: Mo(CO)5 + P(CH3)3 Mo(CO)5P(CH3)3

a. Is the proposed mechanism consistent with the equation for the overall reaction?

b. Identify the intermediate(s).

c. Write the rate law for each step.

3. If the first step is slow compared with the second step, what would you expect to be

the observed rate law?

A + 2B C

rate = k[A]^0[B]^1

K = rate / [A]^0[B]^1 = 0.012/((0.02)^0(0.6)^1) = 0.02 S^-1

rate = 0.02(0.01^0)(0.01^1) = 0.0002 mol L-1 s-1.

2.
a.
Mo(CO)6 -----> Mo(CO)5 + CO

Mo(CO)5 + P(CH3)3 ----> Mo(CO)5P(CH3)3
-------------------------------------------------

Mo(CO)6 + P(CH3)3 -----> Mo(CO)5P(CH3)3 + CO

----------------------------------------------------

yes the mechanism consistent with overall reaction.

b. intermediate : Mo(CO)5

c. 1st step : rate = k [Mo(CO)6]

2nd step : rate = k[Mo(CO)5][P(CH3)3]

3. If the first step is slow compared with the second step.

rate of the reaction depends up on slow step only.

rate = k [Mo(CO)6]

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.