Statement I: The rate law for the reaction is When the concentration of both A and B is doubled, the reaction rate is increased

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Solution

Q.
Given below are two statements: [2024]

Statement I: The rate law for the reaction $A + B \to C$ is $rate (r) = k {[A]}^{2} [B] .$ When the concentration of both A and B is doubled, the reaction rate is increased "x" times.

Statement II:

The figure is showing "the variation in concentration against time plot" for a "y" order reaction.

The value of x + y is _______.

Ans.
(8)

Statement I: $r_{1} = k {[A_{1}]}^{2} [B_{1}]$

$r_{2} = k {[A_{2}]}^{2} [B_{2}] = k {[2 A_{1}]}^{2} [2 B_{1}]$

$\frac{r_{2}}{r_{1}} = \frac{k {[2 A_{1}]}^{2} [2 B_{1}]}{k {[A_{1}]}^{2} [B_{1}]} = 8 = x$

Statement II: For zero order reaction: $[R] = {[R]}_{0} - k t, y = 0$

$x + y = 8$

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