Question

What is δg for the formation of solid uranium hexafluoride from uranium and fluorine at 25∘c when the partial pressure of f2 is 0.054 atm ? the standard free energy of formation of uf6(s) is -2068 kj/mol?

Answer 1

The reaction is

$U(s)+3F_{2} (g)-->UF_{6} (s)$

the Q of reaction will be

$Q = \frac{1}{(pF_{2})^{3}}$

$Q = \frac{1}{(0.054)^{3} } = 6350.66$

Δ$G=$Δ$G^{0}+RTlnQ$

Putting values

ΔG = -2068000 + (8.314)(298)lnQ

ΔG = -2068000 + (8.314)(298)ln(6350.66) = -2046305 J /mol = -2046.3 kJ / mol