If a reaction follows the Arrhenius equation, the plot lnk vs 1/(RT) gives a straight line with a gradient (–y) unit. The energy required to activate the reactant is
If a reaction follows the Arrhenius equation, the plot lnk vs 1/(RT) gives a straight line with a gradient (–y) unit. The energy required to activate the reactant is
-y unit
yR unit
y/R unit
y unit
The Correct Option is A
Solution and Explanation
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Rate law for a reaction between $A$ and $B$ is given by $\mathrm{R}=\mathrm{k}[\mathrm{A}]^{\mathrm{n}}[\mathrm{B}]^{\mathrm{m}}$. If concentration of A is doubled and concentration of B is halved from their initial value, the ratio of new rate of reaction to the initial rate of reaction $\left(\frac{\mathrm{r}_{2}}{\mathrm{r}_{1}}\right)$ is
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