(B) According to Le Chatelier's principle,if the temperature of a system at equilibrium is increased,the system will shift in the direction that a

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Favours the endothermic reaction only

(B) According to Le Chatelier's principle,if the temperature of a system at equilibrium is increased,the system will shift in the direction that absorbs heat to counteract the change. Since endothermic reactions absorb heat $(\Delta H > 0)$,an increase in temperature favours the endothermic reaction. Therefore,the correct option is $(B)$.

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

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Raising the temperature of an equilibrium system:

A
Favours the exothermic reaction only
B
Favours the endothermic reaction only
C
Favours both the exothermic and endothermic reactions
D
Favours neither the exothermic nor endothermic reactions

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6-1.Equilibrium (Chemical Equilibrium)

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Le-Chaterlier principle and It’s application

The yield of product in the reaction $A_{2(g)} + 2B_{(g)} \rightleftharpoons C_{(g)} + Q \ kJ$ would be high at

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For the reaction $Br_2 \rightleftharpoons 2Br$,the equilibrium constants at $500 \, K$ and $700 \, K$ are $1 \times 10^{-10}$ and $1 \times 10^{-5}$ respectively. The reaction is .......

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The equilibrium constant for a reaction,$A + B \rightleftharpoons C + D$ is $1 \times 10^{-2}$ at $298 \ K$ and is $2$ at $273 \ K$. The chemical process resulting in the formation of $C$ and $D$ is

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Which one of the following conditions will favour maximum formation of the product in the reaction
$A_{2(g)} + B_{2(g)} \rightleftharpoons X_{2(g)}; \Delta_{r} H = -X \ kJ$

MediumNEET 2018

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For the formation of $NH_{3(g)}$ from $H_{2(g)}$ and $N_{2(g)}$,which one of the following graphs represents the yield of ammonia at equilibrium? (Assume $T_1 < T_2$,unless mentioned)

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Raising the temperature of an equilibrium system:

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The yield of product in the reaction $A_{2(g)} + 2B_{(g)} \rightleftharpoons C_{(g)} + Q \ kJ$ would be high at

For the reaction $Br_2 \rightleftharpoons 2Br$,the equilibrium constants at $500 \, K$ and $700 \, K$ are $1 \times 10^{-10}$ and $1 \times 10^{-5}$ respectively. The reaction is .......

The equilibrium constant for a reaction,$A + B \rightleftharpoons C + D$ is $1 \times 10^{-2}$ at $298 \ K$ and is $2$ at $273 \ K$. The chemical process resulting in the formation of $C$ and $D$ is

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Which one of the following conditions will favour maximum formation of the product in the reaction
$A_{2(g)} + B_{2(g)} \rightleftharpoons X_{2(g)}; \Delta_{r} H = -X \ kJ$