Consider the following reaction at 283 K: A + B rightarrow C + D where rate = k[

Question

Consider the following reaction at 283 K: A + B rightarrow C + D where rate = k[A][B]. An experiment was performed where [A]_0 = 2.87 M and [B]_0 = 0.00239 M. A plot of In[B] vs. time has a slope of -0.1469. What will the rate of this reaction be when [A] = [B] = 0.713 M? -10 87 M/s Consider the following reaction at 283 K: A + B rightarrow C + D where rate = k[A][B]. An experiment was performed where [A]_0 = 2.87 M and [B]_0 = 0.00239 M. A plot of In[B] vs. time has a slope of -0.1469. What will the rate of this reaction be when [A] = [B] = 0.713 M? -10 87 M/s

Explanation / Answer

A plot of In [B] vs time has slope = k, where k is rate constant

Hence, -k = -0.1469

             k = 0.1469

Given that [A] = [B] = 0.713 M

Hence,     

                rate = k [A] [B]

                  = 0.1469 x 0.713 M x 0.713 M

                      = 0.075 M/s

Therefore,

   rate of reaction = 0.075 M/s

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