Medium
Write the unit of the rate constant for the following reactions:
$1.$ Zero order
$2.$ Second order
$1.$ Zero order
$2.$ Second order
(N/A) The general formula for the unit of the rate constant $(k)$ for a reaction of order $(n)$ is given by: $(mol \ L^{-1})^{1-n} \ s^{-1}$.
$1.$ For a zero-order reaction $(n = 0)$:
Unit $= (mol \ L^{-1})^{1-0} \ s^{-1} = mol \ L^{-1} \ s^{-1}$.
$2.$ For a second-order reaction $(n = 2)$:
Unit $= (mol \ L^{-1})^{1-2} \ s^{-1} = (mol \ L^{-1})^{-1} \ s^{-1} = L \ mol^{-1} \ s^{-1}$.
$1.$ For a zero-order reaction $(n = 0)$:
Unit $= (mol \ L^{-1})^{1-0} \ s^{-1} = mol \ L^{-1} \ s^{-1}$.
$2.$ For a second-order reaction $(n = 2)$:
Unit $= (mol \ L^{-1})^{1-2} \ s^{-1} = (mol \ L^{-1})^{-1} \ s^{-1} = L \ mol^{-1} \ s^{-1}$.
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For a reaction $A$ $\xrightarrow{K_1} B$ $\xrightarrow{K_2} C$. If the rate of formation of $B$ is set to be zero,then the concentration of $B$ is given by:
During the kinetic study of the reaction $2A + B \rightarrow C + D$,the following results were obtained:
Experiment $[A] \ (M), [B] \ (M)$ and Initial rate of formation of $D$ $i. \ [A]=0.1, [B]=0.1$ $6.0 \times 10^{-3} \ M \ s^{-1}$ $ii. \ [A]=0.3, [B]=0.2$ $7.2 \times 10^{-2} \ M \ s^{-1}$ $iii. \ [A]=0.3, [B]=0.4$ $2.88 \times 10^{-1} \ M \ s^{-1}$ $iv. \ [A]=0.4, [B]=0.1$ $2.40 \times 10^{-2} \ M \ s^{-1}$
Based on the above data,the overall order of the reaction is:
| Experiment | $[A] \ (M), [B] \ (M)$ and Initial rate of formation of $D$ |
|---|---|
| $i. \ [A]=0.1, [B]=0.1$ | $6.0 \times 10^{-3} \ M \ s^{-1}$ |
| $ii. \ [A]=0.3, [B]=0.2$ | $7.2 \times 10^{-2} \ M \ s^{-1}$ |
| $iii. \ [A]=0.3, [B]=0.4$ | $2.88 \times 10^{-1} \ M \ s^{-1}$ |
| $iv. \ [A]=0.4, [B]=0.1$ | $2.40 \times 10^{-2} \ M \ s^{-1}$ |
Based on the above data,the overall order of the reaction is:
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