At 298 K , ∆H = 520.0 kJ and ∆S = 184 J/K for the reaction shown below. MnO2(s)  ⟶ Mn(s) + O2(g) (a) Use the data to decide if this reaction is spontaneous at 298 K. (b) What is the temperature above which the reaction is spontaneous?

Which of the following is true when ∆G = 0?

A reaction mixture contains 0.139 M I2, 0.0392 M Cl2, and 0.222 M ICl for the reaction shown below: I2(g) + Cl2(g) ⇌ 2ICl(g)              KC = 9.04 at 298 K Show all your work and setup for credit. A) Calculate QC for the reaction. B) Is the reaction at equilibrium? C) If the reaction is not at equilibrium, will it proceed to form more reactants or more product?

Calculate ΔG°rxn for the following reaction at 525 K. CH2O(g) +  2H2(g) → CH4(g)   +  H2O(g) ΔH° = -94.9 kJ;  ΔS° = -224.2 J/K Answer: ΔG°rxn  = kJ

For the reaction 2A + B + C → D + 2F, the rate law is: rate = k2-1 Which of the following statements is false?

Calculate ΔG°rxn for the following reaction at 298 K. Hg(g) → Hg(l)  ΔH° = -61.4 kJ;  ΔS° = -99.1 J/K Answer: ΔG°rxn  = kJ

Consider the following exothermic equilibrium reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g) Which of the following actions will increase the amount of SO3(g) present at equilibrium?

Predict the sign (∆S > 0 or ∆S < 0) of the entropy change (∆S) for the following processes. (a) CO2(s) ⟶ CO2(g) (b) CaCO3(s) ⟶ CaO(s) + CO2(g) (c) 4Fe(s) + 3O2(g) ⟶ 2Fe2O3(s)

Consider the following reaction, for which Kc = 0.0136 at 731 K 2HI(g) ⇌ H2(g) + I2(g) Which of the following statements is always true, regardless of the conditions (temperature, pressure, etc)?

Predict the sign (∆S > 0 or ∆S < 0) of the entropy change (∆S) for the following processes. (a) NaNO3(s) ⟶ Na+(aq) + NO3-(aq) (b) CaCO3(s) ⟶ CaO(s) + CO2(g) (c) 2C6H14(l) + 19O2(g) ⟶ 14H2O(g) + 12CO2(g)