Using data from Appendix 4, calculate ΔG for the reaction 2 H2 S(g)+SO2(g) ⇌3 Smombic (s)+2 H2

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Using data from Appendix 4, calculate ΔG for the reaction 2...

Using data from Appendix 4, calculate $\Delta G$ for the reaction $$2 \mathrm{H}_{2} \mathrm{~S}(g)+\mathrm{SO}_{2}(g) \rightleftharpoons 3 \mathrm{~S}_{\text {mombic }}(s)+2 \mathrm{H}_{2} \mathrm{O}(g)$$ for the following conditions at $25^{\circ} \mathrm{C}$ : $$\begin{array}{l}P_{\mathrm{H}_{2} \mathrm{~S}}=1.0 \times 10^{-4} \mathrm{~atm} \\P_{\mathrm{SO}_{2}}=1.0 \times 10^{-2} \mathrm{~atm} \\ P_{\mathrm{H}_{2} \mathrm{O}}=3.0 \times 10^{-2} \mathrm{~atm}\end{array}$$

Using data from Appendix 4, calculate $\Delta G$ for the reaction
$$2 \mathrm{H}_{2} \mathrm{~S}(g)+\mathrm{SO}_{2}(g) \rightleftharpoons 3 \mathrm{~S}_{\text {mombic }}(s)+2 \mathrm{H}_{2} \mathrm{O}(g)$$
for the following conditions at $25^{\circ} \mathrm{C}$ :
$$\begin{array}{l}P_{\mathrm{H}_{2} \mathrm{~S}}=1.0 \times 10^{-4} \mathrm{~atm} \\P_{\mathrm{SO}_{2}}=1.0 \times 10^{-2} \mathrm{~atm} \\
P_{\mathrm{H}_{2} \mathrm{O}}=3.0 \times 10^{-2} \mathrm{~atm}\end{array}$$

Key Concepts

The Equation ?G = ?G° + RT ln Q

This equation bridges the standard state free energy change and the actual free energy change when the reaction conditions differ from the standard state. Here, R is the universal gas constant and T is the absolute temperature in Kelvin. The term RT ln Q adjusts ?G° to account for the non-standard pressures or concentrations of the reactants and products, thus providing the true driving force of the reaction under specific conditions.

Reaction Quotient (Q)

The reaction quotient, Q, is a dimensionless number that relates the activities or partial pressures of the products and reactants at any point in time during a reaction. In gaseous systems, the partial pressures are used to compute Q, and it provides insight into how far the reaction has proceeded relative to its equilibrium state.

Gibbs Free Energy Change (?G)

Gibbs free energy change is a thermodynamic quantity that indicates the spontaneity of a chemical reaction under non-standard conditions. It takes into account both the enthalpy and entropy changes in a system to determine whether a reaction will occur spontaneously. A negative ?G means the reaction can proceed without external work, while a positive ?G indicates non-spontaneity under the given conditions.

Standard Gibbs Free Energy Change (?G°)

The standard Gibbs free energy change, ?G°, is the change in free energy when a reaction occurs under standard conditions (typically 1 atm pressure for gases and 1 M concentration for solutions) at a specified temperature. This value serves as a reference point for calculating the free energy change under different conditions.

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