Can someone help me with this question?
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 0.272 M?
2HI(g) ↔ H2(g) + I2(g) Keq = 0.016
The answer is fundamental and you need to understand and remember it.
If ANY of the molar concentrations are INCREASED OR DECREASED, then all of the equilibrium concentrations WILL change BUT, and this is important, Kc WILL NOT CHANGE. After all, a constant is not a constant if it changes so the new Kc will be 0.016. Pressure changes, concentrations changes, volume changes will not change Kc. The only variable that will change Kc is temperature. Increasing or decreasing T will change Kc. Remember that. It's important.