Calculate the standard Gibbs energy of the given reaction at 25°C
CO(g) + half CO +CO2
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.
Calculate the standard Gibbs energy of the given reaction at 25°C
CO(g) + half CO(g) =CO2
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.
To calculate the standard Gibbs energy (ΔG°) of a reaction at a given temperature, we need the standard Gibbs energies of formation (ΔG°f) for all the reactants and products involved. Assuming you meant the reaction:
CO(g) + 1/2 O2(g) + CO2(g) → 2CO2(g)
The standard Gibbs energies of formation for the species involved are as follows:
ΔG°f[CO(g)] = -137.3 kJ/mol
ΔG°f[O2(g)] = 0 kJ/mol (since oxygen gas is the standard reference state)
ΔG°f[CO2(g)] = -394.4 kJ/mol
Now, we can calculate the standard Gibbs energy of the reaction using the following formula:
ΔG° = ∑ΔG°f(products) - ∑ΔG°f(reactants)
Plugging in the values:
ΔG° = [2 × ΔG°f[CO2(g)]] - [ΔG°f[CO(g)] + 1/2 × ΔG°f[O2(g)] + ΔG°f[CO2(g)]]
ΔG° = [2 × (-394.4 kJ/mol)] - [-137.3 kJ/mol + 1/2 × 0 kJ/mol + (-394.4 kJ/mol)]
Simplifying:
ΔG° = -788.8 kJ/mol + 137.3 kJ/mol + 197.2 kJ/mol
ΔG° = -454.3 kJ/mol
Therefore, the standard Gibbs energy of the given reaction at 25°C is approximately -454.3 kJ/mol. Note that the negative value implies that the reaction is spontaneous in the forward direction at this temperature.