Which equilibrium system will show an increase in product formation when the volume is decreased? A. H2 (g) + I2 (g) ⇄ 2HI (g) B. 2NH3 (g) ⇄ N2 (g) + 3H2 (g) C. 2H2 (g) + O2 (g) ⇄ 2H2O (g) D. None of the above

At equilibrium, which of the following reactions will have the largest percentage of reactant remaining? A. CO2 (g) ⇌ 2 CO (g) + O2 (g) Kc = 3 × 10-92 B. 2 NO2 (g) ⇌ N2O4 (g) Kc = 4.70 C. 2 H2 (g) + O2 (g) ⇌ 2 H2O (g) Kc = 3 × 1081 D. H2O (g) + CO (g) ⇌ H2 (g) + CO2 (g) Kc = 24   E. More Information is needed

part b

Write the equilibrium expressions for the following reactions a. 3 Fe (s) + 4 H20 (g) Fe304 (s) + 4 H2 (g) b. 2 SO2 (g) + 02 (g)= 2 SO3 (g)

Consider the exothermic equilibrium reaction: N2(g)+3H2(g)⇌2NH3(l) If the following changes are made to this system at equilibrium, which direction will the reaction shift in order to return to equilibrium? a) If N2 is added? b) If the temperature is increased?

At a certain temperature the reaction CO2(g) + H2(g) ⇄ CO(g) + H2O(g) has Kc = 2.51. If 2.50 mol of carbon monoxide and 2.50 mol of water are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide at equilibrium?