Consider the following reaction at 279 K:
2A + B → C + D
where rate = k[A][B]2. An experiment was performed where [A]o = 2.79 M and [B]o = 0.00233 M. A plot of 1/[B] vs. time has a slope of 10.01. What will the rate of this reaction be when [A] = [B] = 0.387 M?
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Question & Answer: Consider the following reaction at 279 K: 2A + B → C + D…..
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Reaction is 2nd order with respect to B
Hence graph of 1/[B} vs time gives us slope = k
given slope = 10.01 , hence k = 10.01
Rate = k [A] [B]^2
= 10.01 ( 0.387) ( 0.387^2)
= 0.58 M/s