First slide

Order

Question

For the reaction, $A + B \to Products,$ the rate law is given as $rate = K [A] {[B]}^{2}$ . When the concentration of A is doubled and the concentration of B is halved then rate

Easy

A

remains unaffected
B

becomes half
C

Increases by sixteen times
D

Increases by two times

Solution

Let initial concentration of $[A] = [B] = 1 M$
$\begin{array}{l} ∴ r_{initial} = K [1] {[1]}^{2} = K; \\ r_{final} = K [2] {[\frac{1}{2}]}^{2} \\ r_{final} = \frac{1}{2} K; \end{array}$

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