Medium
The given data are for the reaction:
$2NO_{(g)} + Cl_{2(g)} \to 2NOCl_{(g)}$ at $298 \ K$
Experiment $[Cl_2] \ (M)$ $[NO] \ (M)$ Rate $(mol \ L^{-1} \sec^{-1})$ $I$ $0.05$ $0.05$ $1 \times 10^{-3}$ $II$ $0.15$ $0.05$ $3 \times 10^{-3}$ $III$ $0.05$ $0.15$ $9 \times 10^{-3}$
The rate law for the reaction is:
$2NO_{(g)} + Cl_{2(g)} \to 2NOCl_{(g)}$ at $298 \ K$
| Experiment | $[Cl_2] \ (M)$ | $[NO] \ (M)$ | Rate $(mol \ L^{-1} \sec^{-1})$ |
| $I$ | $0.05$ | $0.05$ | $1 \times 10^{-3}$ |
| $II$ | $0.15$ | $0.05$ | $3 \times 10^{-3}$ |
| $III$ | $0.05$ | $0.15$ | $9 \times 10^{-3}$ |
The rate law for the reaction is:
- A$r = k[NO][Cl_2]$
- B$r = k[Cl_2][NO]^2$
- C$r = k[Cl_2]^2[NO]$
- D$r = k[Cl_2]$
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Similar Questions
The experimental data for the reaction $2A + B_2 \longrightarrow 2AB$ is given below:
Exp. $[A] \ (mol \ L^{-1})$ $[B_2] \ (mol \ L^{-1})$ Rate $(mol \ L^{-1} \ S^{-1})$ $1$ $0.50$ $0.50$ $1.6 \times 10^{-4}$ $2$ $0.50$ $1.00$ $3.2 \times 10^{-4}$ $3$ $1.00$ $1.00$ $3.2 \times 10^{-4}$
Determine the rate law for the reaction.
| Exp. | $[A] \ (mol \ L^{-1})$ | $[B_2] \ (mol \ L^{-1})$ | Rate $(mol \ L^{-1} \ S^{-1})$ |
|---|---|---|---|
| $1$ | $0.50$ | $0.50$ | $1.6 \times 10^{-4}$ |
| $2$ | $0.50$ | $1.00$ | $3.2 \times 10^{-4}$ |
| $3$ | $1.00$ | $1.00$ | $3.2 \times 10^{-4}$ |
Determine the rate law for the reaction.
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