Please refer to the image provided.
7) The equilibrium constant for the following reaction is 5.0 at 400°C. CO(g) + H2(g) ⇌ CO2(g) + H2O(g). Determine the direction of the reaction if the following amount (in moles) of each compound is placed in a 1.0 L flask: CO = 0.50, H2O = 0.40, CO2 = 0.80, H2 = 0.90.
a) 0.01, 0.02, 0.03, 0.04
b) 1.22, 1.22, 2.78, 2.78
c) 0.61, 1.22, 1.39, 2.39
8) The equilibrium concentrations of [O2] = 0.21 Molar and [O3] = 6.0 x 10^-8 Molar, calculate the value of Kc for the reaction: 2O3(g) ⇌ 3O2(g).
9) At a particular temperature, a 2.0 L flask contains 2.0 mol H2S, 0.40 mol H2, and 0.80 mol S2. Calculate Kc at this temperature for the reaction: H2S(g) + S2(g) ⇌ H2(g) + S2(g).
10) The following equilibrium pressures were observed for the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g). PNH3 = 3.1x10^3 atm, PN2 = 8.5x10 atm, PH2 = 3.1x10 atm. Calculate the value for the equilibrium constant Kp.
11) For the equilibrium: CH4(g) ⇌ H2(g) + C(g), if the initial concentration of CH4 is 0.0300 M and the equilibrium concentration of H2 is 0.01375 M:
a) Calculate the equilibrium concentrations of CH4 and H2.
b) Determine the numerical value of Kc.
12) If the equilibrium partial pressures are PCO2 = 0.0387 atm and PNH3 = 0.0774 atm, what is the value of Kp for the reaction: CO2(g) + 2NH3(g) ⇌ H2CO3(g) + NH3(g).
