Calculate ΔG∘ at 298 K for the following reactions.

A) Ca(s)+CO2(g)+12O2(g)→CaCO3(s)

B) 2KClO3(s)→2KCl(s)+3O2(g)

C) CO(g)+H2O(g)→H2(g)+CO2(g)

To calculate the standard Gibbs free energy change (ΔG∘) at 298 K for each reaction, we need to use the equation:

ΔG∘ = ΔH∘ - TΔS∘

Where:
ΔH∘ = standard enthalpy change
ΔS∘ = standard entropy change
T = temperature in Kelvin (298 K in this case)

Let's calculate ΔG∘ for each reaction:

A) Ca(s) + CO2(g) + 1/2O2(g) → CaCO3(s)

First, we need to find the standard enthalpy change (ΔH∘) and standard entropy change (ΔS∘) from reference sources or experimental data.

Assuming we have the ΔH∘ = -1206.9 kJ/mol and ΔS∘ = 92.9 J/(mol·K) for this reaction, we can proceed with the calculation:

ΔG∘ = ΔH∘ - TΔS∘
ΔG∘ = -1206.9 kJ/mol - (298 K) * (-92.9 J/(mol·K))

Note: We need to convert ΔS∘ from J/(mol·K) to kJ/(mol·K) to match the units of ΔH∘.

B) 2KClO3(s) → 2KCl(s) + 3O2(g)

Assuming we have the ΔH∘ = 0 kJ/mol and ΔS∘ = 84.67 J/(mol·K) for this reaction, we can proceed with the calculation:

ΔG∘ = ΔH∘ - TΔS∘
ΔG∘ = 0 kJ/mol - (298 K) * (-84.67 J/(mol·K))

C) CO(g) + H2O(g) → H2(g) + CO2(g)

Assuming we have the ΔH∘ = 41.2 kJ/mol and ΔS∘ = 92.6 J/(mol·K) for this reaction, we can proceed with the calculation:

ΔG∘ = ΔH∘ - TΔS∘
ΔG∘ = 41.2 kJ/mol - (298 K) * (-92.6 J/(mol·K))

Please note that the actual values of ΔH∘ and ΔS∘ may vary depending on the reference source used, so it is important to double-check with reliable sources or experimental data.

dGorxn = (n*dGo products) - (n*dGo reactants)