The equation for the reaction in the figure b | vedclass

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(D) At the instant $3 	ext{ min}$,the concentration of $H_2$ shows a sudden vertical spike,indicating that $H_2$ was added to the system.According to

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Hydrogen was added

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(D) At the instant $3 	ext{ min}$,the concentration of $H_2$ shows a sudden vertical spike,indicating that $H_2$ was added to the system.According to Le Chatelier's principle,adding a reactant shifts the equilibrium in the forward direction to consume the excess reactant.Consequently,the concentration of $H_2$ decreases from its peak,the concentration of $I_2$ decreases,and the concentration of $HI$ increases until a new equilibrium is established.Therefore,the correct change is that hydrogen was added.

The equation for the reaction in the figure below is: $H_{2(g)} + I_{2(g)} + \text{heat} \rightleftharpoons 2HI_{(g)}$
At the instant $3 \text{ min}$,what change was imposed on the equilibrium?

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The equation for the reaction in the figure below is: $H_{2(g)} + I_{2(g)} + \text{heat} \rightleftharpoons 2HI_{(g)}$At the instant $3 \text{ min}$,what change was imposed on the equilibrium?