For the reaction H_{2(g)} + I_{2(g)} rightlef | vedclass

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(A) For a general reaction $aA + bB \rightarrow cC + dD$,the rate of reaction is given by: Rate $= -\frac{1}{a} \frac{\Delta [A]}{\Delta t} = -\frac{1

Vedclass · Accepted Answer

$-\frac{\Delta [H_2]}{\Delta t} = -\frac{\Delta [I_2]}{\Delta t} = \frac{1}{2} \frac{\Delta [HI]}{\Delta t}$

Vedclass · Answer

(A) For a general reaction $aA + bB \rightarrow cC + dD$,the rate of reaction is given by: Rate $= -\frac{1}{a} \frac{\Delta [A]}{\Delta t} = -\frac{1}{b} \frac{\Delta [B]}{\Delta t} = \frac{1}{c} \frac{\Delta [C]}{\Delta t} = \frac{1}{d} \frac{\Delta [D]}{\Delta t}$. For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,the stoichiometric coefficients are $1, 1, 2$ respectively. Thus,the rate of reaction is expressed as: Rate $= -\frac{\Delta [H_2]}{\Delta t} = -\frac{\Delta [I_2]}{\Delta t} = \frac{1}{2} \frac{\Delta [HI]}{\Delta t}$.

For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,the rate of reaction is expressed as:

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