Chemical EquilibriumHard
Question
For the reaction H2(g) + I2(g) $\rightleftharpoons$2HI(g), the rate law expression is
Options
A.$- \frac{1}{2}.\frac{d\lbrack HI\rbrack}{dt} = K_{- 1}\lbrack HI\rbrack^{2} - K_{1}\left\lbrack H_{2} \right\rbrack\left\lbrack I_{2} \right\rbrack$
B.$- \frac{1}{2}.\frac{d\lbrack HI\rbrack}{dt} = \frac{K_{1}\lbrack HI\rbrack^{2}}{K_{- 1}\left\lbrack H_{2} \right\rbrack\left\lbrack I_{2} \right\rbrack}$
C.$- \frac{1}{2}.\frac{d\lbrack HI\rbrack}{dt} = K_{1}\left\lbrack H_{2} \right\rbrack\left\lbrack I_{2} \right\rbrack - K_{- 1}\lbrack HI\rbrack^{2}$
D.$- \frac{1}{2}.\frac{d\lbrack HI\rbrack}{dt} = K_{1}K_{- 1}\left\lbrack H_{2} \right\rbrack\left\lbrack I_{2} \right\rbrack$
Solution
Net rate of reaction of HI,
$- \frac{1}{2}.\frac{d\lbrack HI\rbrack}{dt} = r_{b} - r_{f} = K_{- 1}\lbrack HI\rbrack^{2} - K_{1}\left\lbrack H_{2} \right\rbrack\left\lbrack I_{2} \right\rbrack$
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