contestada

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.

Respuesta :

superman1987
we can get ΔG from this formula:

ΔG = -R*T*(㏑K)

when K = p(N2O4) / p(NO2)^2

we have P(N2O4) = 1.64 atm 

and P(NO2)^2 = 0.38 atm 

by substitution:

             =1.64 atm / (0.38)^2

            = 11.36

and R = 8.314

and T = 298 K

so by substitution on ΔG formula:

∴ ΔG = 8.314 *298 *(㏑ 11.36)

        = - 6020.7 

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

Gibbs free energy formula,

[tex]\rm \bold { \Delta G = R \times T}[/tex]

Where,

R - gas constant = 8.314 J/K/mole

T - temperature in Kelvin = 298 K

Put the value, we get

[tex]\rm \bold { \Delta G = - 6020.7 }[/tex]

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

To know more about free energy, refer to the link:

https://brainly.com/question/15319033?referrer=searchResults

Otras preguntas