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)

Are the following solutions acidic, basic, or neutral? a) KBr(aq) b) NH4Br(aq) c) NaNO2(aq)

Calculate ΔSsurr at 298 K. 2NO(g) +  O2(g) → 2NO2(g) ΔH = -114 kJ

Determine the Kb for CN- at 25°C. The Ka for HCN is 4.9 × 10-10.

1. Select the strongest acid from the following: A) HNO3 or HNO2 B) HCl or HBr 2. Select the strongest base from the following: C) ClO- or ClO2- 3. Which will be more soluble in an acidic solution? D) PbCl2 or PbF2

For the titration of 15.0 mL of 0.200 M HCl with 0.200 M NaOH. HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) a) What is the initial pH? pH =  b) What is the pH after the addition of 5.00 mL of NaOH ? pH =  c) What is the pH after the addition of 15.0 mL of NaOH? pH =  d) What is the pH after the addition of 20.0 mL of NaOH? pH =