Consider the reaction 2no2(g) → n2o4(g) and δg∘(no2(g)) = 51.84 kj/mol, δg∘(n2o4(g)) = 98.28 kj/mol. calculate δg at 298 k if the partial pressures of no2 and n2o4 are 0.38atm and 1.64atm , respectively.

The Gibbs free energy for the reaction is -6020.7 J/mol.

Gibbs free energy formula,

Where,

R - gas constant = 8.314 J/K/mole

T - temperature in Kelvin = 298 K

Put the value, we get

Hence we can say that the Gibbs free energy for the reaction is -6020.7 J/mol.

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i think it is d. e because the next one is igneous.

gold is my favorite solid.