A reaction is of first order in reactant A and of second order in reactant B. How is the rate of this reaction affected when (i) the concentration of B alone is increased to three times (ii) the concentrations of A as well as B are doubled?
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According to the given reaction:
Rate = k [A] [B]2
(i) When the concentration of reactant ‘B’ is increased three times the rate of reaction becomes 9 times.
i.e., Rate = k [A] [3B]2 = 9k[A] [B]2
(ii) When the concentration of reactants A and B are doubled, then rate becomes 8 times.
i.e., Rate = k [2A]1 [2B]2 = 8k[A] [B]2
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