For a gaseous reaction, standard conditions are 298 k and a partial pressure of 1 atm for all species. for the reaction c2h6(g)+h2(g)↽−−⇀2ch4(g) the standard change in gibbs free energy is δ°=−32.8 kj/mol . what is δg for this reaction at 298 k when the partial pressures are =0.250 atm , =0.300 atm , and =0.800 atm ?

ΔG = -27.5 kJ/mol

Explanation:

The given reaction is:

The Gibbs free energy (ΔG) is related to the standard gibbs free energy (ΔG°) as follows:

where R = gas constant

T = temperature

Q = reaction quotient

For the given reaction:

Here:

ΔG°=-32.8 kJ/mol

R = 0.008314 kJ/mol-K

T = 298 K

P(CH4) = 0.800 atm

P(C2H6) = 0.250 atm

P(H2) = 0.300 atm