Answer:
A nonspontaneous process
Explanation:
The spontaneity of a reaction is given by the standard Gibbs free energy (ΔG°). We can calculate ΔG° using the following expression.
ΔG° = ∑np . ΔG°f(p) - ∑nr . ΔG°f(r)
where,
ni are the moles of reactants and products
ΔG°f(p) are the standard Gibbs free energies of formation of reactants and products
For the equation,
CO₂(g) → CO₂(aq)
ΔG° = 1 mol × ΔG°f(CO₂(aq)) - 1 mol × ΔG°f(CO₂(g))
ΔG° = 1 mol × (-386.0 kJ/mol) - 1 mol × (-394.4 kJ/mol)
ΔG° = 8.4 kJ
By convention, ΔG° > 0 means that the reaction is nonspontaneous.
Ca(s)+ H2O (l)----->H2 +Ca(oH)2
Ca(s)+2H2O(l)----->H2(g)+Ca(oH)2
I hope this helps
sorry if it's wrong
Answer:
D
Explanation:
it goes past the decimal three places
I think the correct answer is D
