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Chemistry
Tutor: None Selected Time limit: 1 Day

An equilibrium mixture, at 672°C in a 1155-mL container, involving the chemical system

N2(g) + 3H2(g)  2NH3(g)

is found to contain 9.14 g of N2, 0.707 g of H2, and 0.300 g of NH3. Calculate the equilibrium constant (Keq expressed in terms of the molar concentrations) at the given temperature.

A 5.00-L vessel contained 4.61×10-2 mol of gaseous PCl3, 5.22×10-2 mol of gaseous PCl5, and 6.83×10-2 mol of Cl2 gas at equilibrium at 222°C. 
Calculate the value of Keq (expressed in terms of the molar concentrations) for the reaction

PCl3(g) + Cl2(g)  PCl5(g)

May 8th, 2015

  1. SOLUTION

    First, write K (equilibrium constant expression) in terms of activities.

    K=(aNH3)2(aN2)(aH2)3

    Then, replace the activities with the partial pressures in the equilibrium constant expression.

    Kp=(PNH3)2(PN2)(PH2)3

    Finally, substitute the given partial pressures into the equation.

    Kp=(0.003)2(0.094)(0.039)3=1.61mol/l

  2. Keq = [PCl5] / [PCl3][Cl2] = 0.0103 / 0.00832 x 0.0119 = 104

May 8th, 2015

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