(A) For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,the number of moles of gaseous reactants is $1 + 1 = 2$ and the number of mole

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(A) For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,the number of moles of gaseous reactants is $1 + 1 = 2$ and the number of moles of gaseous products is $2$. Since the change in the number of moles of gas $(\Delta n_g = 2 - 2 = 0)$ is zero,the equilibrium position is not affected by a change in pressure or volume. Therefore,the reaction direction does not change.

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

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$H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$. In this reaction,when pressure increases,the reaction direction:

A
Does not change
B
Forward
C
Backward
D
Decrease

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6-1.Equilibrium (Chemical Equilibrium)

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Le-Chaterlier principle and It’s application

Adding an inert gas to the system $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ at equilibrium at constant volume will lead to:

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In which of the following reactions does the yield of the product not increase by the application of high pressure?

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In a reversible reaction,a catalyst will affect the rate of

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In what manner will an increase of pressure affect the following equilibrium equation?
$C_{(s)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + H_{2(g)}$

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Under which conditions of temperature and pressure is the dissociation of molecular hydrogen into atomic hydrogen favored?

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$H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$. In this reaction,when pressure increases,the reaction direction:

Similar Questions

Adding an inert gas to the system $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ at equilibrium at constant volume will lead to:

In which of the following reactions does the yield of the product not increase by the application of high pressure?

In a reversible reaction,a catalyst will affect the rate of

In what manner will an increase of pressure affect the following equilibrium equation?$C_{(s)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + H_{2(g)}$

Under which conditions of temperature and pressure is the dissociation of molecular hydrogen into atomic hydrogen favored?

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In what manner will an increase of pressure affect the following equilibrium equation?
$C_{(s)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + H_{2(g)}$