Applications of Thermodynamics

Which of the following best describes the 'system' in thermodynamics?

Which process leads to an increase in entropy ($S°$)?

Given the following standard molar entropies: $S°(N_2(g)) = 191.6 \frac{J}{mol \cdot K}$, $S°(H_2(g)) = 130.7 \frac{J}{mol \cdot K}$, and $S°(NH_3(g)) = 192.3 \frac{J}{mol \cdot K}$, calculate the standard entropy change ($ΔS°$) for the reaction: $N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)$

If a reaction has a Gibbs Free Energy change of $ΔG° = -50 \frac{kJ}{mol}$, the reaction is:

Calculate the standard Gibbs Free Energy change ($ΔG°$) at 298 K for a reaction where the standard enthalpy change ($ΔH°$) is -100 kJ/mol and the standard entropy change ($ΔS°$) is -50 J/(mol·K).

The standard Gibbs Free Energy change ($ΔG°$) for a reaction is $+25 \frac{kJ}{mol}$ at 298 K. Calculate the equilibrium constant (K) for this reaction. (R = 8.314 J/(mol·K))

A reaction has a positive $ΔH°$ and a negative $ΔS°$. How will increasing the temperature affect the spontaneity of the reaction?

Which of the following is a characteristic of a galvanic cell?

Calculate the cell potential ($E°_{cell}$) for a galvanic cell composed of the following two half-reactions: $Zn^{2+}(aq) + 2e^- \rightarrow Zn(s)$, $E° = -0.76 V$ $Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$, $E° = +0.34 V$

For a redox reaction, the cell potential ($E°$) is +0.50 V at 298 K. Calculate the standard Gibbs Free Energy change ($ΔG°$) for the reaction if two electrons are transferred (n = 2). (F = 96485 C/mol)