(a) For a reaction A + B → P, the rate is given by Rate = k[A] [B]2(i) How is the rate of reaction affected if the concentration of B is doubled?(ii) What is the overall order of reaction if A is present in large excess?(b) A first order reaction takes 30 minutes for 50% completion. Calculate the time required for 90% completion of this reaction. (log 2 = 0.3010)
(a) For a reaction A + B → P, the rate is given by Rate = k[A] [B]2(i) How is the rate of reaction affected if the concentration of B is doubled?(ii) What is the overall order of reaction if A is present in large excess?(b) A first order reaction takes 30 minutes for 50% completion. Calculate the time required for 90% completion of this reaction. (log 2 = 0.3010)
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Question
(a) For a reaction A + B → P, the rate is given by Rate = k[A] [B]2
(i) How is the
(ii) What is the overall order of reaction if A is present in large excess?
(b) A first order reaction takes 30 minutes for 50% completion. Calculate the time required for 90% completion of this reaction. (log 2 = 0.3010)
Expert Solution
Step 1
Given,
rate of reaction,
where, [A] is the concentration of A, and [b] is the concentration of B, k is constant.
Now,
i)
concentration of B is doubled,
[B'] = [2B]
So new rate will be,
Step 2
ii)
A is present in large excess
If A is present in large excess, then rate will independent of A, that is new rate of reaction will be,
So, the order of rate is 2
Step by step
Solved in 4 steps
