PREDICT EFFECT OF FOLLOWING CHANGE ON THE AMOUNTOF PRODUCT:A2(g)+B2(g) sign of reversible reaction A2B2 1.a gaseous catalyst is used 2.Argon is used3.volume of vessel is increased. ((please explain with answer))
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1. Any catalyst changes the rate of the reaction, but never changes the free energy and equilibrium. So the equilibrium will remain same.
2.In case of use of Argon, 2 cases arise, 1st in case of constant volume, and another in case of constant pressure. Please check this in any class 12 chemistry book. I don't remember this.
3. Increase in vessel volume leads to decrease in concentration of both reactants and products. So the equilibrium remains same.
Explanation:
please check the 2nd answer from book.
Hope you will be able to understand.
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