1. The reaction shown below has the rate law: Rate = k [BrO3–][Br–][H+]. BrO3–(
ID: 698858 • Letter: 1
Question
1. The reaction shown below has the rate law: Rate = k[BrO3–][Br–][H+].
BrO3–(aq) + 5 Br–(aq) + 6 H+(aq) 3 Br2(aq) + 3 H2O(l)
What is the overall order of reaction?
zeroth
first
second
third
2.
The following set of data was obtained by the method of initial rates for the reaction:
(H3C)3CBr + OH- (H3C)3COH + Br-
What is the value of the rate constant, k?
8.8 × 10-4 s-1
4.4 × 10-4 s-1
1.8 × 10-4 s-1
A.zeroth
B.first
C.second
D.third
2.
The following set of data was obtained by the method of initial rates for the reaction:
(H3C)3CBr + OH- (H3C)3COH + Br-
What is the value of the rate constant, k?
A.8.8 × 10-4 s-1
B.4.4 × 10-4 s-1
C.1.8 × 10-4 s-1
Explanation / Answer
1. Option D, since order is equal to the sum of powers of the reactants present in the rate law equation. Here powers on BrO3-, Br- and H+ are 1, 1 and 1 respectively. So, sum of these is 1+1+1= 3
Hence third order reaction.
2. Data is insufficient
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