Consider the following gas phase equilibrium in a vessel of a constant volume: 2

Question

Consider the following gas phase equilibrium in a vessel of a constant volume: 2AB(g) A_2(g) + B_2(g) K = 0.400 We initially have a concentration of 1.00 M AB, 0.100 M A_2 and 0.200M B_2. Calculate the initial value of Q 2AB(g) A_2(g) + B_2(g) If the change in A_2 concentration is +x, what is the charge in AB concentration? +2x -2x -x +x 2AB(g) A_2(g) + B_2(g) K = 0.400 Which initial concentrations of 1.00 M AB, 0.100M A_2 and 0 200M B_2 and a charge of +x in the concentration of A_2, what is the equilibrium concentration of AB in terms of x? 1.00 - 2x 1.00 - x -2x -x 2AB(g) A_2(g) + B_2(g) K = 0.400 With initial concentrations of 1.00 M AB, 0.100M A_2 and 0.200M B_2, what is the equilibrium value of x? [This will require you to use the quadratic equation.] 2AB(g) A_2(g) + B_2(g) K = 0.400 With initial concentration of 1.00 M AB, 0.100M A_2 and 0.200M B_2. What is the equilibrium value of [AB]? A reaction has a K = 1.0 times 10^-3 at 35 degree C and 2.5 times 10^-2 at 25 degree C. The reaction is Endothermic Exothermic Cannot tell Gaseous. A particular reaction has K = 0.0800 at 25 degree C. calculate delta G degree in kJ (or kJ/mol) A reaction has DG degree of 22.3 kJ (or kJ/mol) at 25 degree. Calculate K For a particular reaction, K = 0.00133 at 25 degree C and K = 0.0133 at 125 degree C. Calculate delta H degree in kJ (or kJ/mol) If a reaction has a K = 0.100 at 500, degree_K and delta H degree = -25.2 kJ (or kJ/mol), what would K be at 600^degree K [I use^degree K here to distinguish temperature from the symbol for the equilibrium constant, but that is old-fashioned] Click Save and Submit to save and submit. Click Save All Answers to save all answers.

Explanation / Answer

1. For the given reaction

Q=[A2][B2]/[AB]2

Q=0.0200

2. B

Change in AB=-2x

3. A

At equilibrium [AB]=1-2x

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