1) Consider the following equilibrium: CO (g) + H2O (g) 4 CO2 (g) + H2 (g)

11.60 moles CO and11.60 moles H2O are placed in a 12.00L container at 690o C Kp=10.0. Calculate all equilibrium moles

2) Consider the following equilibrium: SbCl5(g) 4 SbCl3(g)+ Cl2(g)

Starting with 0.265 moles SbCl3, 0.300 moles Cl2 and 0.225 moles SbCl5, in a 3.50 liter closed container. Calculate all equilibrium moles Keq = 2.50x10-12 at 256 C

3) Calculate the pH of a solution with the following: 5.12 moles of HCl are placed in a 3.00 L of water

4) Given the acid pKa is 4.76. Calculate the pH of a 0.35M acetic acid solution:

5) Given the reaction below, calculate G when equilibrium is reached

CH4 + O2 H2O + CO2