Consider the following equilibrium (K_c = 2.68 × 10⁻³ at 800 °C):

CaCO₃ (s) ⇌ CaO (s) + CO₂ (g)

Is the formation of products favored at equilibrium? What is/are the relative concentration/s of the species involved at equilibrium?

Consider the following equilibrium:

F₂ (g) ⇌ 2 F (g); K_eq = 7.40×10⁻¹³ at 500 Kelvin

Calculate [F₂] at equilibrium when [F] = 5.25 × 10⁻⁴ M.

Consider the equilibrium reaction shown in the image below:

Calculate the value of K for the reaction.

The ΔH of the following reaction is 228 kcal/mol (953 kJ/mol). 

2 Cs(g) + Br₂(l) → 2 CsBr(s)

Does the entropy of the reaction decrease or increase? Why?

Determine the system whose entropy is increasing. 

The reaction Z(s) → X(g) + Y(g) is depicted in the following figure.

Assuming the reaction has ΔH = 52.4 kJ/mol (12.5 kcal/mol), will the reaction be spontaneous at high temperatures?

Plotted on the energy diagram below are blue and orange curves. Identify the curve that represents a nonspontaneous reaction and a spontaneous reaction.

Consider the following reaction:

NH₃(l) ⇌ NH₃(g)

The ΔH and ΔS for the reaction above are 23.3 kJ/mol (5.57 kcal/mol) and 97.3 J/mol•K (23.2 cal/mol•K), respectively. Is the reaction favored or unfavored by ΔH? By ΔS?