1. the equilibrium will not shift, because while the total pressure will raise, the concentrations will still be the same (the same amount of mols of each gas per volume) since the volume did not change
2. it will shift to the left. there are 4 mols of gas on the left, and 2 mols of gas on the right side. when you lower the pressure, according to la chatelier's principle, the equilibrium will tend to conteract (ie, the pressure will try to go back up). in order for the pressure to go back up, the equilibrium shifts to the left because there are more mol of gas on the left
3. false, because when you add water, the concentrations will change, which effects the equilibrium
4. false, from, la chatelier's principle, in order to counteract the increase in H2 concentration, more H2 will react, meaning more I2 will react, meaning hte equilibrium shifts to the right
5. adding heat will make it shift to the left because that's how the extra heat would be counteracted. if it is shifting to the left, is the equilibrium constant be higher or lower than Kc?
