Which of the following expression is correct for the reaction given below?
$2HI(g) \rightarrow H_2(g) + I_2(g)

Question

Which of the following expression is correct for the reaction given below?
$2HI(g) \rightarrow H_2(g) + I_2(g)$

Accepted Answer

For the reaction $2HI(g) ightarrow H_2(g) + I_2(g)$, the rate of the reaction is expressed as:
$	ext{Rate} = -\frac{1}{2} \frac{\Delta[HI]}{\Delta t} = +\frac{\Delta[H_2]}{\Delta t} = +\frac{\Delta[I_2]}{\Delta t}$
From this relationship, we can equate the rate of disappearance of $HI$ with the rate of appearance of $H_2$:
$-\frac{1}{2}\frac{\Delta[HI]}{\Delta t} = \frac{\Delta[H_2]}{\Delta t}$
Rearranging this gives:
$-\frac{\Delta[HI]}{\Delta t} = 2\frac{\Delta[H_2]}{\Delta t}$

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