(B) The reaction is $A_{(g)} + \frac{1}{2} B_{(g)} \rightleftharpoons C_{(g)} + \text{heat}$.Since the reaction releases heat,it is an exothermic reac

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(B) The reaction is $A_{(g)} + \frac{1}{2} B_{(g)} \rightleftharpoons C_{(g)} + \text{heat}$.Since the reaction releases heat,it is an exothermic reaction.According to Le Chatelier's principle,low temperature favors the forward direction for exothermic reactions.Calculate the change in the number of gaseous moles: $\Delta n_g = 1 - (1 + 0.5) = -0.5$.Since $\Delta n_g Therefore,high pressure is favorable for the forward reaction.

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

Medium

For a reaction $A_{(g)} + \frac{1}{2} B_{(g)} \rightleftharpoons C_{(g)} + \text{heat}$,favorable conditions for the reaction to occur in the forward direction are:

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A
Low $T$ and Low $P$
B
Low $T$ and high $P$
C
High $T$ and Low $P$
D
High $T$ and high $P$

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6-1.Equilibrium (Chemical Equilibrium)

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Le-Chaterlier principle and It’s application

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Consider the following reversible reaction at equilibrium,$2H_2O_{(g)} \rightleftharpoons 2H_{2(g)} + O_{2(g)}$; $\Delta H = 241.7 \ kJ$. Which one of the following changes in conditions will lead to maximum decomposition of $H_2O_{(g)}$?

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In which of the following gaseous equilibrium will an increase in pressure increase the yield of the products?

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In which of the following reactions will a change in pressure not affect the rate of reaction?

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For the chemical reaction: $BaO_{2(s)} \rightleftharpoons BaO_{(s)} + \frac{1}{2} O_{2(g)}$,$\Delta H = +ve$. At equilibrium,the pressure of $O_2$ depends upon:

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State the optimum pressure and temperature for the production of ammonia by the Haber process.

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For a reaction $A_{(g)} + \frac{1}{2} B_{(g)} \rightleftharpoons C_{(g)} + \text{heat}$,favorable conditions for the reaction to occur in the forward direction are:

Similar Questions

Consider the following reversible reaction at equilibrium,$2H_2O_{(g)} \rightleftharpoons 2H_{2(g)} + O_{2(g)}$; $\Delta H = 241.7 \ kJ$. Which one of the following changes in conditions will lead to maximum decomposition of $H_2O_{(g)}$?

In which of the following gaseous equilibrium will an increase in pressure increase the yield of the products?

In which of the following reactions will a change in pressure not affect the rate of reaction?

For the chemical reaction: $BaO_{2(s)} \rightleftharpoons BaO_{(s)} + \frac{1}{2} O_{2(g)}$,$\Delta H = +ve$. At equilibrium,the pressure of $O_2$ depends upon:

State the optimum pressure and temperature for the production of ammonia by the Haber process.

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