I need help with some AP chem problems, thanks in advance!

Question

Consider the reaction shown below. Which of the following changes would cause the equilibrium to shift 

     left?

CaCO3 (s) + H2SO4 (aq) ↔ CaSO4 (s) + H2O (l) + CO2 (g)   ΔH = -122 kJ

(A) Carbon dioxide gas is removed

(B) The reaction is heated 

(C) The volume of the reaction vessel is increased

(D) Water is added 

2. Initially there are only reactant particles in a sealed vessel. Which of the following statements regarding the    

     system is correct? 

1. The system must shift to the right to reach equilibrium.
2. A shift for the reaction cannot be determined without knowing the value of the quotient, Q
3. A shift in the reaction cannot be determined without knowing the value of the equilibrium constant, K
4. The reaction must be at equilibrium.

3. For the reaction shown below, if all gases are initially present at equal partial pressure, which of the 

     following statements is correct?

CO (g) + 2H2 (g) ↔ CH3OH (g) Kp = 1.0 x 103

(A) The reaction must shift to the left to increase the partial pressures of the reactants

(B) The reaction is at equilibrium

(C) The reaction must shift to the right to increase the partial pressure of the product

(D) This cannot be determined without the exact value of the partial pressures.

Answer 1

I can help you solve these questions yourself, but I will not give you the answers. What is your timeline?