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For the reaction below, the thermodynamic equilibrium constant is KP = 0.000708 at 30 C. NH4CO2NH2(s) 2 NH3(g) + CO2(g) Suppose that 0.008 moles of...
For the reaction below, the thermodynamic equilibrium constant is KP = 0.000708 at 30 °C.
NH4CO2NH2(s) → 2 NH3(g) + CO2(g)
Suppose that 0.008 moles of NH4CO2NH2, 0.016 moles of NH3, and 0.008 moles of CO2 are added to a 7.0 L container at 30 °C.
(a) What are QP and ΔGR for the initial reaction mixture? QP = ; ΔGR = kJ mol−1
(b) What is the total equilibrium pressure in the 7.0 L container at 30 °C? [Hint: Set up an I.C.E. table and then show that the equilibrium partial pressure of NH3 will be two times the equilibrium partial pressure of CO2.]
