N2(g) + 3 H2(g) yields 2 NH3(g)

If the volume of the container in which the above equilibrium had been established were to be halved, then when equilibrium is reestablished the

a. moles of N2 increase
b. moles of NH3 increase
c. moles of NH3 decrease
d. moles of NH3 stay the same

explanation would be helpful

Question

N2(g) + 3 H2(g)  yields 2 NH3(g)

If the volume of the container in which the above equilibrium had been established were to be halved, then when equilibrium is reestablished the

a. moles of N2 increase
b. moles of NH3 increase
c. moles of NH3 decrease
d. moles of NH3 stay the same

explanation would be helpful

abmon98 · Answer

If the Volume is Halved If at Constant Temperature then Pressure would be Doubled and Equilbrium would Shift to the side where there are less number of Moles therefore Yield of Ammonia Increase. At constant Pressure,Temperature (Direct Proportion Relation) would Also Decrease, Manufacturing of ammonia is an exothermic Process and favours decrease in temperature so equilbrium would shift to the products and more of ammonia is produced . I think the answer is B