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Consider the following reaction at 283 K: 1 A + 1 B → C + D, where the rate = k[A]²[B]. An experiment was performed for a certain number of seconds where [A]₀ = 0.00117 M and [B]₀ = 1.44 M. A plot of 1/A vs. time gave a straight line with a slope of 8.83. What will the rate of this reaction be if a new experiment is performed where [A] = [B] = 0.58 M?
Sagot :
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