${\text {Rate}=\frac{d R}{d T}}$
${=\alpha[A]^{x} \cdot[B]^{y}}$
${=k[A]^{x} \cdot[B]^{y}}$
$\mathrm{K}=$ rate constant
Rate, $r_{1}=k[A]^{2}[B]^{3}$
On doubling the concentration, we have
$r_{2}=k[2 A]^{2}[2 B]^{3}$
$=32 k[A]^{2}[B]^{3}=32 r_{1}$
[લો; $R =8.314 \,J\, mol ^{-1}\, K ^{-1}$ In $3.555=1.268$]
${A}+{B} \rightarrow {M}+{N}$ $......$ ${kJ} {mol}^{-1}$ બરાબર છે. (નજીકના પૂર્ણાંકમાં)