1. GENERAL CHEMISTRY-II (1412)
S.I. # 17
1. Write the Keq for the reaction:
NiCO3 (s) + 2H+ (aq)   Ni2+ (aq) + CO2(g) + H2O (l)
2. Write (Kc) Equilibrium constant for
AgCl (s) + 2 NH3(aq)  [Ag(NH3)2]+ (aq) + Cl- (aq)
3. Gaseous hydrogen Iodide is placed in a closed1.0 L container at 425°C where it
partially decomposes to hydrogen and iodine. 2HI (g)  H2 (g) + I2 (g). At
equilibrium, it is found that PH I =3.53x10-3 atm and PH2 = 4.79x10-4 atm, PI2 =
4.79x10-4. What is the value of Keq at this temperature?
4. What is the value of equilibrium constant Keqif at equilibrium PH2 = 6.5x10-7 atm,
PI2 = 1.06x10-5 atm, PHI = 1.87x10-5 atm. 2HI (g)  H2 (g) + I2 (g).
5. Calculate the equilibrium constant for the reaction below if a 3.25 L tank is
found to contain 0.343 atm O2, 0.0212 atm SO3, and 0.00419 atm SO2.
2SO3 (g)  2 SO2 (g) + O2 (g)
6. A mix of 0.10 mol of NO, 0.050 mol of H2, and 0.10 mol of H2O is placed in a 1.0 L

2. vessel at 300K. At equilibrium PNO = 0.062, calculate the equilibrium concentrations
of H2, N2 and H2O and Kc.
2NO (g) + 2H2 (g)  N2 (g) + 2H2O (g)
7. A mixture of 0.2000 mol of CO2, 0.1000 mol of H2 and 0.1600 mol of H2O is
placed in a 2.000 L vessel. The following equilibrium is established at 500K:
CO2(g) + H2(g)  CO(g) + H2O (g)
a) calculate the initial partial pressures of CO2, H2 and H2O.
b) At equilibrium PH2O = 3.51 atm. Calculate the equilibrium partial pressures of
CO2, H2 and CO.
c) Calculate Kp for the reaction.