(B) The dissolution of sodium sulphate is an exothermic process,which can be represented as: $Na_2SO_4(s) + aq \rightleftharpoons Na_2SO_4(aq) + \text

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Some solid will precipitate out from the solution

(B) The dissolution of sodium sulphate is an exothermic process,which can be represented as: $Na_2SO_4(s) + aq \rightleftharpoons Na_2SO_4(aq) + \text{Heat}$.According to Le Chatelier's principle,if the temperature of an exothermic system at equilibrium is increased,the equilibrium will shift in the direction that absorbs the excess heat,which is the reverse direction.Therefore,the reverse reaction occurs,causing some of the dissolved $Na_2SO_4$ to precipitate out of the solution.

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

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Sodium sulphate dissolves in water with the evolution of heat. Consider a saturated solution of sodium sulphate. If the temperature is raised,then according to Le Chatelier's principle:

A
More solid will dissolve
B
Some solid will precipitate out from the solution
C
The solution will become supersaturated
D
Solution concentration will remain unchanged

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6-1.Equilibrium (Chemical Equilibrium)

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Le-Chaterlier principle and It’s application

For the following reaction,which change will shift the equilibrium towards the product?
$I_{2(g)} \rightleftharpoons 2I_{(g)}; \Delta H_r^o(298 \ K) = +150 \ kJ$

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In the reaction $A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)}$,the backward reaction is favoured by

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Suppose the reaction $PCl_{5(s)} \rightleftharpoons PCl_{3(s)} + Cl_{2(g)}$ is in a closed vessel at equilibrium. What is the effect on the equilibrium concentration of $Cl_{2(g)}$ by adding $PCl_{5(s)}$ at constant temperature?

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For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,in which direction will the equilibrium shift if an inert gas is added at constant pressure?

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When $I_2$ dissociates to its atomic form the following reaction occurs:
$I_{2(g)} \rightleftharpoons 2I_{(g)} ; \Delta_r H^o = +150 \ kJ \ mol^{-1}$
The forward reaction is favoured at:

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Sodium sulphate dissolves in water with the evolution of heat. Consider a saturated solution of sodium sulphate. If the temperature is raised,then according to Le Chatelier's principle:

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For the following reaction,which change will shift the equilibrium towards the product?$I_{2(g)} \rightleftharpoons 2I_{(g)}; \Delta H_r^o(298 \ K) = +150 \ kJ$

In the reaction $A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)}$,the backward reaction is favoured by

Suppose the reaction $PCl_{5(s)} \rightleftharpoons PCl_{3(s)} + Cl_{2(g)}$ is in a closed vessel at equilibrium. What is the effect on the equilibrium concentration of $Cl_{2(g)}$ by adding $PCl_{5(s)}$ at constant temperature?

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,in which direction will the equilibrium shift if an inert gas is added at constant pressure?

When $I_2$ dissociates to its atomic form the following reaction occurs:$I_{2(g)} \rightleftharpoons 2I_{(g)} ; \Delta_r H^o = +150 \ kJ \ mol^{-1}$The forward reaction is favoured at:

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For the following reaction,which change will shift the equilibrium towards the product?
$I_{2(g)} \rightleftharpoons 2I_{(g)}; \Delta H_r^o(298 \ K) = +150 \ kJ$

When $I_2$ dissociates to its atomic form the following reaction occurs:
$I_{2(g)} \rightleftharpoons 2I_{(g)} ; \Delta_r H^o = +150 \ kJ \ mol^{-1}$
The forward reaction is favoured at: