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Standard XII

Chemistry

Le Chatelier's Principle for Del N Equals to 0

Given the rea...

Question

Given the reaction $A \to B + C$ , when $△ H_{r e a c t i o n}$ is negative, what effect would increase in 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 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 reached is exothermic. So, if temperature is increased then as per Le Chaterlier's principle, the equilibrium shifts to left side (backward direction).

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Given the reaction A→B+C, when △Hreaction is negative, what effect would increase in 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 reached is exothermic. So, if temperature is increased then as per Le Chaterlier's principle, the equilibrium shifts to left side (backward direction).

Given the reaction $A \to B + C$ , when $△ H_{r e a c t i o n}$ is negative, what effect would increase in 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 reached is exothermic. So, if temperature is increased then as per Le Chaterlier's principle, the equilibrium shifts to left side (backward direction).