(B) Given $K_c > K_p$. Using the relation $K_p = K_c(RT)^{\Delta n}$,we have $(RT)^{\Delta n} < 1$,which implies $\Delta n < 0$. Since $\Delta n < 0$,

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Increasing pressure and temperature

(B) Given $K_c > K_p$. Using the relation $K_p = K_c(RT)^{\Delta n}$,we have $(RT)^{\Delta n} Since $\Delta n Given $\Delta H = +40 \ kcal$,the reaction is endothermic. According to Le Chatelier's principle,increasing the temperature favors the forward (endothermic) reaction. Therefore,the product yield increases on increasing temperature and increasing pressure.

Class 11 Chemistry 1 Equilibrium: Chemical Equilibrium Le-Chaterlier principle and It’s application

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In a reversible reaction at $300 \ K$,$K_c > K_p$ and $\Delta H = +40 \ kcal$. The product will be obtained in a higher amount on:

A
Decreasing pressure and temperature
B
Increasing pressure and temperature
C
Decreasing pressure and increasing temperature
D
Decreasing temperature and increasing pressure

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Class 11

Chemistry Questions

Chapter

1 Equilibrium: Chemical Equilibrium

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Le-Chaterlier principle and It’s application

In which of the following equilibrium reactions,the equilibrium would shift to the right,if total pressure is increased?

Medium

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The binding of oxygen by haemoglobin $(Hb)$ forming $(HbO_2)$ is partially regulated by the concentration of $H_3O^{+}$ and dissolved $CO_2$ in blood.
$HbO_2 + H_3O^{+} + CO_2 \rightleftharpoons (H^{+} - Hb - CO_2) + O_2 + H_2O$
Release of $O_2$ is favoured when there is:

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If pressure increases,what is the effect on the given equilibrium $C_{(s)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + H_{2(g)}$?

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For the reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$,$\Delta H^o = -198 \, kJ$. According to Le Chatelier's principle,the favorable conditions for the forward reaction are:

Easy

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For the balanced reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g) + \text{Heat}$,which of the following conditions will favor the forward reaction?

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In a reversible reaction at $300 \ K$,$K_c > K_p$ and $\Delta H = +40 \ kcal$. The product will be obtained in a higher amount on:

Similar Questions

In which of the following equilibrium reactions,the equilibrium would shift to the right,if total pressure is increased?

The binding of oxygen by haemoglobin $(Hb)$ forming $(HbO_2)$ is partially regulated by the concentration of $H_3O^{+}$ and dissolved $CO_2$ in blood.$HbO_2 + H_3O^{+} + CO_2 \rightleftharpoons (H^{+} - Hb - CO_2) + O_2 + H_2O$Release of $O_2$ is favoured when there is:

If pressure increases,what is the effect on the given equilibrium $C_{(s)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + H_{2(g)}$?

For the reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$,$\Delta H^o = -198 \, kJ$. According to Le Chatelier's principle,the favorable conditions for the forward reaction are:

For the balanced reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g) + \text{Heat}$,which of the following conditions will favor the forward reaction?

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The binding of oxygen by haemoglobin $(Hb)$ forming $(HbO_2)$ is partially regulated by the concentration of $H_3O^{+}$ and dissolved $CO_2$ in blood.
$HbO_2 + H_3O^{+} + CO_2 \rightleftharpoons (H^{+} - Hb - CO_2) + O_2 + H_2O$
Release of $O_2$ is favoured when there is: