- #1
sgstudent
- 739
- 3
When I have a reaction CO(g)+2H2(g) <=> CH3OH if I increas the concentration of CO, the equilibrium will be shifted to the right so more methanol will form. However, in that process won't the concentration of Hydrogen gas decrease? So won't that cause a change in equilibrium as well? If so, how would it affect the equilibrium
Also for ionic Salts like NaCl(s) <=> Na+ (aq)+Cl- (aq), how will increasing the NaCl affect the equilibrium? Because I'm not sure what's the concentration of pure solids. Also, I think this explains why solubility decreases with concentration but I can't seem to understand why that happens using Le Chatelier's principle here.
Hope you guys can help me out here :)
Also for ionic Salts like NaCl(s) <=> Na+ (aq)+Cl- (aq), how will increasing the NaCl affect the equilibrium? Because I'm not sure what's the concentration of pure solids. Also, I think this explains why solubility decreases with concentration but I can't seem to understand why that happens using Le Chatelier's principle here.
Hope you guys can help me out here :)