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Standard XII

Chemistry

Law of Mass Action

Given the rea...

Question

Given the reaction $A \to B + C$ , where $△ H_{r x n}$ is negative, what effect would increasing the temperature (at constant pressure) have on the system at equilibrium?

No change

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Cannot be determined

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Shift to the right

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Shift to the left for K < 1 and to the right for K > 1

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Shift to the left

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Solution

The correct option is E Shift to the left
Given reaction is :-
$A \to B + C; △ H < 0$
Here, forward reaction is exothermic. So, if temperature is increased then as per Le Chatelier's principle, the equilibrium shifts to left side (backward direction).

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Given the reaction A→B+C, where △Hrxn is negative, what effect would increasing the temperature (at constant pressure) have on the system at equilibrium?

The correct option is E Shift to the leftGiven reaction is :-A→B+C;△H<0Here, forward reaction is exothermic. So, if temperature is increased then as per Le Chatelier's principle, the equilibrium shifts to left side (backward direction).

Given the reaction $A \to B + C$ , where $△ H_{r x n}$ is negative, what effect would increasing the temperature (at constant pressure) have on the system at equilibrium?

The correct option is E Shift to the left
Given reaction is :-
$A \to B + C; △ H < 0$
Here, forward reaction is exothermic. So, if temperature is increased then as per Le Chatelier's principle, the equilibrium shifts to left side (backward direction).