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

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(A) For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2 HI_{(g)}$,the reactants $H_2$ and $I_2$ are consumed to form the product $HI$.Therefore

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(A) For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2 HI_{(g)}$,the reactants $H_2$ and $I_2$ are consumed to form the product $HI$.Therefore,the molar concentration of reactants ($H_2$ and $I_2$) decreases over time until equilibrium is reached.Simultaneously,the molar concentration of the product $(HI)$ increases over time until equilibrium is reached.Once equilibrium is attained,the concentrations of all reactants and products remain constant over time.This behavior is correctly represented by the graph where the curves for $H_2$ and $I_2$ show a downward trend and the curve for $HI$ shows an upward trend,all leveling off at the same time.

For the reaction,$H_{2(g)} + I_{2(g)} \rightleftharpoons 2 HI_{(g)}$,the attainment of equilibrium is predicted correctly by:

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