1. The problem statement, all variables and given/known data The following reaction is at equilibrium at one atmosphere, in a closed container NaOH(s) + CO2(g)-> NaHCO3 (s) which, if any, of the following actions will decrease the total amount of CO2 gas present at equilibrium? 1)decreasing the volume of the container 2) none of the above 3) removing half of the solid NaHCO3 4)adding mlore solid NaOH 5)adding N2 gas to double the pressure 3. The attempt at a solution I chose (1) and got it wrong, so I chose (5) next but it was wrong again, I thought that solid is not included in equilibrium constant which means that it has little effect on equilibrium change, that's why I eliminated (3) and (4). I guess for, (1), decreasing the volume wouldn't do much to shift the equilibrium constant to the right.. then I don't understand why (5) is wrong because if you add more gas, it will double the pressure thus makeing the reactants to shift to the right to re-establish the equilibrium constant,, Is the answer none of the above? Please help!