Question

Use the standard free energy of formation data in Appendix G to determine the free energy change for each of the following reactions, which are run under standard state conditions and 25 °C. Identify each as either spontaneous or nonspontaneous at these conditions.

A) MnO₂ (s) → Mn(s) + O₂(g)

B) H₂(g) + Br₂(l) → 2HBr(g)

C) Cu(s) + S(g) → CuS(s)

D) 2LiOH(s) + C0₂(g) → Li₂C0₃(s)+H₂O(g)

Answer 1

To determine the spontaneity of the reactions, we need to calculate the standard free energy change for each reaction and identify whether it is spontaneous or nonspontaneous.

We can use the standard free energy of formation data from Appendix G for this calculation.

By comparing the calculated ΔG° values with zero, we can determine if the reactions are spontaneous or nonspontaneous at standard state conditions and 25 °C.

Step-by-step explanation:

First, we need to calculate the standard free energy change (ΔG°) for each reaction using the standard free energy of formation data from Appendix G.

The equation for calculating ΔG° is:

ΔG° = ΔG°(products) - ΔG°(reactants)

Once we have calculated ΔG°, we can determine if the reaction is spontaneous or nonspontaneous at standard state conditions and 25 °C. If ΔG° is negative, the reaction is spontaneous.

If ΔG° is positive, the reaction is nonspontaneous.

Let's calculate ΔG° for each reaction:

(a) MnO2 (s) → Mn (s) + O2 (g)

ΔG° = ΔG°(Mn) + ΔG°(O2) - ΔG°(MnO2)

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