2HI(g) ↔ H2(g) + I2(g) Keq = 0.016

Initially a container contains 0.13 M HI and no product. What is the equilibrium concentration of H2?

For the reaction:

2HI(g) ↔ H2(g) + I2(g) Keq = 0.016

Initially a container contains 0.60 M HI, 0.038 M H2, and 0.15 M I2 at equilibrium. What is the new equilibrium concentration of H2, if the H2 concentration is increased by 0.228 M?

Question

2HI(g) ↔ H2(g) + I2(g) Keq = 0.016

Initially a container contains 0.13 M HI and no product. What is the equilibrium concentration of H2?


For the reaction: 

2HI(g) ↔ H2(g) + I2(g) Keq = 0.016

Initially a container contains 0.60 M HI, 0.038 M H2, and 0.15 M I2 at equilibrium. What is the new equilibrium concentration of H2, if the H2 concentration is increased by 0.228 M?