Statement 1 : An equation where two gas molecules combine to form one gas molecule in equilibrium will increase the yield of the product when the pressure is increased.
Statement 2 : Increased pressure always favors products.

Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.

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Both Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.

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Statement 1 is correct but Statement 2 is not correct.

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Statement 1 is not correct but Statement 2 is correct.

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Both the Statement 1 and Statement 2 are not correct.

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Solution

The correct option is C
Statement 1 is correct but Statement 2 is not correct.

According to Le Chatelier's principle, a change in pressure, temperature or concentration of the reactant will shift the reaction in a direction so as to counteract the effect of the change. Hence, an increase in pressure will shift the equillibrium in a direction that produces fewer moles of gases. Hence Statement 1 is correct.

However, it is possible that the moles of the reactant is greater than that of the products as in a combination reaction. Hence it is not necessary that increased pressure will always favor the products which leads to Statement 2 being incorrect

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Statement 1 : An equation where two gas molecules combine to form one gas molecule in equilibrium will increase the yield of the product when the pressure is increased.Statement 2 : Increased pressure always favors products.

Statement 1 : An equation where two gas molecules combine to form one gas molecule in equilibrium will increase the yield of the product when the pressure is increased.
Statement 2 : Increased pressure always favors products.