Question

Calculate the standard Gibbs energy of the given reaction at 25°C
CO(g) + half CO +CO2

Answer 1

It is unclear what the products of this reaction are, as the expression provided is incomplete. Please double-check the given chemical equation and provide the full reaction for an accurate calculation of the standard Gibbs energy.

Answer 2

Calculate the standard Gibbs energy of the given reaction at 25°C
CO(g) + half CO(g) =CO2

Answer 3

The chemical equation is not balanced, but assuming the balanced equation is:

CO(g) + 1/2 O2(g) → CO2(g)

The standard Gibbs energy change (ΔG°) can be calculated using the following equation:

ΔG° = ΣnΔG°f(products) - ΣnΔG°f(reactants)

where Σn is the sum of the stoichiometric coefficients, and ΔG°f is the standard Gibbs energy of formation for each species at 25°C and 1 atm.

Using standard Gibbs energy of formation values from a table, we have:

ΔG°f(CO2) = -394.36 kJ/mol
ΔG°f(CO) = -137.27 kJ/mol
ΔG°f(O2) = 0 kJ/mol

Substituting these values into the equation and solving, we get:

ΔG° = (1 × -394.36 kJ/mol) - [1 × -137.27 kJ/mol + 1/2 × 0 kJ/mol]
ΔG° = -394.36 kJ/mol + 137.27 kJ/mol
ΔG° = -257.09 kJ/mol

Therefore, the standard Gibbs energy change for this reaction at 25°C is -257.09 kJ/mol.