(C) The given reaction is $I_{2(g)} \rightleftharpoons 2I_{(g)}$ with $\Delta H_r^o = +150 \ kJ$.Since $\Delta H_r^o > 0$,the reaction is endothermic.

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(C) The given reaction is $I_{2(g)} \rightleftharpoons 2I_{(g)}$ with $\Delta H_r^o = +150 \ kJ$.Since $\Delta H_r^o > 0$,the reaction is endothermic.According to Le Chatelier's principle,for an endothermic reaction,an increase in temperature shifts the equilibrium towards the product side (forward direction) to absorb the excess heat.

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

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Which of the following changes will shift the reaction towards the product?
$I_{2(g)} \rightleftharpoons 2I_{(g)}$ $\Delta H_r^o(298 \ K) = +150 \ kJ$

A
Increase in concentration of $I$
B
Decrease in concentration of $I_2$
C
Increase in temperature
D
Increase in total pressure

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6-1.Equilibrium (Chemical Equilibrium)

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Le-Chaterlier principle and It’s application

What is the effect of increasing pressure on the dissociation of $PCl_5$ according to the equation $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)} - x \ cal$?

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For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,the forward reaction at constant temperature is favoured by

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In the equilibrium $2A_{(g)} + 3B_{(g)} \rightleftharpoons 3C_{(g)} + 2D_{(g)}$,an increase in pressure will:

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Observe the following equilibrium:
$Fe^{3+}_{(aq)} + SCN^{-}_{(aq)} \rightleftharpoons [Fe(SCN)]^{2+}_{(aq)}$
(yellow) (colorless) (deep red)
Addition of aqueous oxalic acid solution to the above equilibrium:

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$N_2$ and $O_2$ combine to form nitric oxide as follows: ${N_2}_{(g)} + {O_2}_{(g)} \rightleftharpoons 2NO - \text{heat}$. Which of the following conditions will favor the production of $NO$?

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Which of the following changes will shift the reaction towards the product?$I_{2(g)} \rightleftharpoons 2I_{(g)}$ $\Delta H_r^o(298 \ K) = +150 \ kJ$

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What is the effect of increasing pressure on the dissociation of $PCl_5$ according to the equation $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)} - x \ cal$?

For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,the forward reaction at constant temperature is favoured by

In the equilibrium $2A_{(g)} + 3B_{(g)} \rightleftharpoons 3C_{(g)} + 2D_{(g)}$,an increase in pressure will:

Observe the following equilibrium:$Fe^{3+}_{(aq)} + SCN^{-}_{(aq)} \rightleftharpoons [Fe(SCN)]^{2+}_{(aq)}$(yellow) (colorless) (deep red)Addition of aqueous oxalic acid solution to the above equilibrium:

$N_2$ and $O_2$ combine to form nitric oxide as follows: ${N_2}_{(g)} + {O_2}_{(g)} \rightleftharpoons 2NO - \text{heat}$. Which of the following conditions will favor the production of $NO$?

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Which of the following changes will shift the reaction towards the product?
$I_{2(g)} \rightleftharpoons 2I_{(g)}$ $\Delta H_r^o(298 \ K) = +150 \ kJ$

Observe the following equilibrium:
$Fe^{3+}_{(aq)} + SCN^{-}_{(aq)} \rightleftharpoons [Fe(SCN)]^{2+}_{(aq)}$
(yellow) (colorless) (deep red)
Addition of aqueous oxalic acid solution to the above equilibrium: