A student ran the following reaction in the laboratory at 636 K:

2HI(g) -> H2(g) + I2(g)

When she introduced 0.316 moles of HI(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 3.12×10-2 M.

Calculate the equilibrium constant, Kc, she obtained for this reaction.

Kc =

Liquid ammonia is produced at high temperatures and under great pressure in a tank by passing a mixture of nitrogen gas and hydrogen gas over an iron catalyst. the reaction is represented by the following equation. n2(g) + 3h2(g) → 2nh3(g) changing all but one experimental condition will affect the amount of ammonia produced. that condition is a) increasing the concentration of both reactants b) changing the temperature within the tank c) decreasing the pressure within the tank. d) increasing only the amount of nitrogen present.