Question

For the reaction : $X\left(g\right)\to Y\left(g\right)+Z9g)$, the following data were obtaned at ${30}^{\circ C}$

Experiment	[X] $\left(mol{L}^{-1}\right)$	Rate $\left(mol{L}^{-1}h{r}^{-1}\right)$
I	0.17	0.05
II	0.34	0.10
III	0.68	0.20

The equilibrium constant for the reaction is 0.50. Assuming that the reaction proceeds by one-step mechanism. Find the rate constant of reverse reaction ?

• A. 0.294 $h{r}^{-1}$
• B. 0.588 $h{r}^{-1}$
• C. 0.123 $h{r}^{-1}$
• D. 0.117 $h{r}^{-1}$

Answer 1

The correct option is B 0.588 $h{r}^{-1}$

$X\left(g\right)\rightleftharpoons Y\left(g\right)+Z\left(g\right)$
$k_{eq}=\frac{k_f}{k_b}$
$\Rightarrow K_b=\frac{0.294h{r}^{-1}}{0.50}=0.588h{r}^{-1}$