Co2(g)+ccl4(g)⇌2cocl2(g) calculate δg for this reaction at 25 ∘c under these conditions: pco2pccl4pcocl2===0.140 atm0.185 atm0.735 atm 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.

The for the reaction is 54.425 kJ/mol

Explanation:

For the given balanced chemical equation:

We are given:

To calculate for the reaction, we use the equation:

For the given equation:

Putting values in above equation, we get:

Conversion factor used = 1 kJ = 1000 J

The expression of for the given reaction:

We are given:

Putting values in above equation, we get:

To calculate the gibbs free energy of the reaction, we use the equation:

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 = 20.85

Putting values in above equation, we get:

Hence, the for the reaction is 54.425 kJ/mol

your answer is a. the enthalpy of formation for a pure element in its standard state is always positive.