During the kinetic study of the reaction, 2 A+B arrow C+D , following results were obtained: Run [A]/ mol L^ -1 [ B]/ mol L^ -1 Initial rate of formation of D/ mol L^ -1 min^ -1 I 0.1 0.1 6.0 ×10^ -1 II 0.3 0.2 7.2 ×10^

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Correct answer: D. rate =k[ A][B]^ 2

In case of (II) and (III) Keeping concentration of [A] constant, when the concentration of [B] is doubled, the rate quadruples. Hence it is second order with respect to B . In case of I \ IV Keeping the concentration of [B] constant, when the concentration of [A] is increased four times, rate also increases four times. Hence, the order with respect to A is one. Hence Rate =k[ A][B]^ 2

During the kinetic study of the reaction, 2 A+B arrow C+D ,...

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Run	{[A]/ mol L^{-1}}	{[ B]/ mol L^{-1}}	Initial rate of formation of D/ mol L^{-1} min^{-1}
I	0.1	0.1	6.0 \times10^{-1}
II	0.3	0.2	7.2 \times10^{-1}
III	0.3	0.4	28.8 \times10^{-1}
IV	0.4	0.1	24.0 \times10^{-1}