Consider the following reaction: co2(g)+ccl4(g)⇌2cocl2(g) calculate δg for this reaction at25 ∘c under these conditions: pco2pccl4pcocl2===0.140atm0.180atm0 .760atm δg∘f for co2(g) is −394.4kj/mol, δg∘f for ccl4(g) is −62.3kj/mol, and δg∘f for cocl2(g) is −204.9kj/mol. express the energy change in kilojoules per mole to one decimal place.

The for the reaction is 54.6 kJ/mol

Explanation:

For the given balanced chemical equation:

We are given:

For the given equation:

Putting values in above equation, we get:

Conversion factor used = 1 kJ = 1000 J

We are given:

Putting values in above equation, we get:

where,

= Gibbs' free energy of the reaction = ?

= Standard gibbs' free energy change of the reaction = 46900 J

R = Gas constant =

T = Temperature =

= equilibrium constant in terms of partial pressure = 22.92

Putting values in above equation, we get:

Hence, the for the reaction is 54.6 kJ/mol