A reaction is first order in A and second order in B.
(i) Write differential rate equation.
(ii) How is the rate affected if the concentration of B is tripled?
(iii) How is the rate affected when the concentrations of both A and B are doubled?
What is the significance of rate constant in the rate expression?

Solution

A reaction is first order in A and second order in B.

(i) $Rate = k {[A]}^{1} {[B]}^{2}$

$(ii) r_{0} = k {[A]}^{1} {[B]}^{2} r_{1} = k {[A]}^{1} {[3 B]}^{2} ∴ r_{1} = 9 \times r_{0}$

$(iii) r_{0} = k {[A]}^{1} {[B]}^{2} r_{2} = k {[2 A]}^{1} {[2 B]}^{2} ∴ r_{2} = 8 \times r_{0}$

Rate constant of a reaction is equal to the rate of reaction when concentration of each of the reactant is unity.

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Some More Questions From Chemical Kinetics Chapter

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Mock Test Series

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