# 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

https://brainmass.com/chemistry/chemical-equilibrium/finding-equilibrium-constant-delta-g-228905

#### Solution Preview

Hi,

here is the answer

Part A

The relation between standard free energy change and equilibrium constant is

∆G_°=-2.303RT ...

#### Solution Summary

This solution is comprised of answers related with Finding equilibrium constant and delta G.

calculate the equilibrium constant Kp

The water - gas shift reaction plays an important role in the production of clean fuel from coal.

CO(g) + H20(g) <--> CO2(g) + H2 (g)

Given Data:

Substance = CO(g) H20(g) CO2(g) H2(g)

Delta H (KJ/Mol) -110.5 -241.8 -393.5 0

Delta S (J/Mol K) 197.7 188.8 213.7 130.7

Use the given data to find the equilibrium constant Kp at 700K?

I know that I am supposed to use the equation:

ln K = Delta G /-R*T. But I am having trouble with the set up required to solve for G using:

Delta G = sum n* delta G products - sum m* reactants.