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Question

Which of the following change will shift the reaction towards the product?
I2(g)2I(g), ΔHr(298K)=+150kJ

A
Increase in concentration of I(g)
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B
Decrease in concentration of I2(g)
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C
Increase in temperature
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D
Increase in total pressure
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Solution

The correct option is C Increase in temperature
The reaction is I2(g)2I(g),ΔHr(298K)=+150kJ.
According to Le-Chatelier's principle, the conditions favouring the formation of I are given below:
(i) High concentration of I2(g).
(ii) High temperature (reaction is endothermic so, on increasing the temperature equilibrium it will shift in the direction where heat is absorbed).
(iii) Low pressure (moles of products are more than moles of reactant. Therefore, if pressure is increased, equilibrium will shift in the direction where moles are decreasing).

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