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Finding the value of the equilibrium constant.

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For the reaction below, the partial pressures of gases at equilibrium are as follows:

H2=7.1x10^-5 atm, Cl2=2.5x10^-6 atm, and HCl=3.0atm. What is the value of the equilibrium constant Kp?

H2(g)+Cl2(g) = 2HCl(g)

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Similar Posting

Finding Equilibrium Constant and Delta G

Part 1:
Ammonia can be produced by the reaction of hydrogen gas and nitrogen gas, as shown below:

N2(g) + 3H2(g) → 2NH3(g)

Given that the standard free energy of formation (∆Gof) of NH3 (g) is -111 kJ/mol at 335 K, calculate the equilibrium constant, K, at this temperature.
To express an answer in exponential notation, use E to indicate the exponent. For example, 3.0 x 103 would be written, 3.0E3.

Part 2:
In the previous question, you had to calculate the the standard Free Energy Change (∆Go) in order to solve for the equilibrium constant, K, for the reaction:

N2(g) + 3H2(g) → 2NH3(g)

This is the Free Energy measured under standard conditions, when the reaction is started with 1.0 M of each of the three gases present. Calculate the non-standard Free Energy change (∆G) at 298 K, given the following non-standard initial concentrations of the three gases (Answer in kJ).
∆Gfo = -16.6 kJ/mol for NH3 (g) at 298 K

initial concentration (M)
N2 1.0
H2 0.09
NH3 4.1

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