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Question

Formula: $a A+b B ightarrow c C+d D$

${	ext {Rate}=\frac{d R}{d T}}$

${=\alpha[A]^{x} \cdot[B]^{y}}$

${=k[A]^{x} \cdot[B]^{y}}$

$\mathr

Vedclass · Accepted Answer

$32$

Vedclass · Answer

Formula: $a A+b B ightarrow c C+d D$

${	ext {Rate}=\frac{d R}{d T}}$

${=\alpha[A]^{x} \cdot[B]^{y}}$

${=k[A]^{x} \cdot[B]^{y}}$

$\mathrm{K}=$ rate constant

Rate, $r_{1}=k[A]^{2}[B]^{3}$

On doubling the concentration, we have

$r_{2}=k[2 A]^{2}[2 B]^{3}$

$=32 k[A]^{2}[B]^{3}=32 r_{1}$

For a reaction between $A$ and $B$ the order with respect to $A$ is $2$ and the other with respect to $B$ is $3.$ The concentrations of both $A$ and $B$ are doubled, the rate will increase by a factor of

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