(C) The given reaction is $H_2 \rightleftharpoons H + H$. Since $\Delta H = +ve$,the reaction is endothermic. According to Le Chatelier's principle,an

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$3500 \, ^{\circ}C$ temperature and $1 \, mm$ pressure

(C) The given reaction is $H_2 \rightleftharpoons H + H$. Since $\Delta H = +ve$,the reaction is endothermic. According to Le Chatelier's principle,an increase in temperature favors the endothermic direction. Also,the number of moles of gas increases from $1$ to $2$ in the forward reaction. Therefore,a decrease in pressure favors the forward reaction. Thus,high temperature and low pressure are favorable conditions.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Le-Chaterlier principle and It’s application

Medium

Which of the following conditions is favorable for the forward reaction in the equilibrium: $H_2 \rightleftharpoons H + H$ $(\Delta H = +ve)$?

A
$2000 \, ^{\circ}C$ temperature and $760 \, mm$ pressure
B
$3500 \, ^{\circ}C$ temperature and $100 \, cm$ pressure
C
$3500 \, ^{\circ}C$ temperature and $1 \, mm$ pressure
D
All are incorrect

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6-1.Equilibrium (Chemical Equilibrium)

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Le-Chaterlier principle and It’s application

The exothermic formation of $ClF_3$ is represented by the equation $Cl_{2(g)} + 3F_{2(g)} \rightleftharpoons 2ClF_{3(g)}$; $\Delta H = -329 \ kJ$. Which of the following will increase the quantity of $ClF_3$ in an equilibrium mixture of $Cl_2, F_2$ and $ClF_3$?

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Consider the reaction equilibrium,$2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$; $\Delta H^\circ = -198 \ kJ$. On the basis of Le Chatelier's principle,the condition favourable for the forward reaction is

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For the reversible reaction,
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + \text{heat}$
The equilibrium shifts in the forward direction:

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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?

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$A$ container at equilibrium contains $SO_3, SO_2$ and $O_2$. The total pressure in the container is increased while the temperature and volume remain constant. According to Le Chatelier's principle,the dissociation of $SO_3$ will........

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Which of the following conditions is favorable for the forward reaction in the equilibrium: $H_2 \rightleftharpoons H + H$ $(\Delta H = +ve)$?

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The exothermic formation of $ClF_3$ is represented by the equation $Cl_{2(g)} + 3F_{2(g)} \rightleftharpoons 2ClF_{3(g)}$; $\Delta H = -329 \ kJ$. Which of the following will increase the quantity of $ClF_3$ in an equilibrium mixture of $Cl_2, F_2$ and $ClF_3$?

Consider the reaction equilibrium,$2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$; $\Delta H^\circ = -198 \ kJ$. On the basis of Le Chatelier's principle,the condition favourable for the forward reaction is

For the reversible reaction,$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + \text{heat}$The equilibrium shifts in the forward direction:

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?

$A$ container at equilibrium contains $SO_3, SO_2$ and $O_2$. The total pressure in the container is increased while the temperature and volume remain constant. According to Le Chatelier's principle,the dissociation of $SO_3$ will........

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For the reversible reaction,
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + \text{heat}$
The equilibrium shifts in the forward direction:

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?