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(a) Consider the reaction $R\rightarrow P$ for which the change in concentration of $R$ with time is shown by the following graph :

(i) Predict the order of reaction.

(ii) What does the slope of the curve indicate ?

(b) The rate of reaction quadruples when temperature changes from $293\; K$ to $313\; K$ . Calculate $E_{a}$ assuming that it does not change with time. $\left [ R=8.314\; JK^{-1\; mol^{-1}} \right ]$

Answers (1)

(a) Order =zero (0)

slope = -K

$\left [ R \right ]=-Kt+\left [ R \right ]$

(b) $E_{a }=?$

$T_{1}=293\; K\; \; \; \; \; T_{2}=313\; K$

$log\frac{K_{2}}{K_{1}}=\frac{E_{a}}{2.303R}\left [ \frac{T_{2}-T_{1}}{T_{1}T_{2}} \right ]$

$K_{2}=4K_{1}$

$log \frac{4K_{1}}{K_{1}}=\frac{E_{a}}{2.303\times 8.314}\left [ \frac{313-293}{(313)(293)} \right ]$

$log \; 4=\frac{20\times E_{a}}{2.303\times 8.314\times 313\times 293}$

$E_{a}=\frac{0.6021\times 2.303\times 8.314\times 313\times 293}{20}$

$E_{a}=52863.33\; J/mol$

Posted by

Sumit Saini

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