At 298 K , ∆H = 58.1 kJ and ∆S = 165 J/K for the reaction shown below. Cu2O(s)  +  C(s) ⟶ 2Cu(s) + CO(g) (a) Use the data to decide if this reaction is spontaneous at 298 K. [a] (b) What is the temperature above which the reaction is spontaneous? [b]

Consider the following redox reaction in acidic solution: Pb4+(aq)  +  Br- (aq) → Pb2+ (aq)  +  BrO3-(aq) When the equation is balanced with smallest whole number coefficients, the coefficient for — (a) Pb4+  = [a] (b) Br-  = [b] (c) Pb2+  = [c] (d) BrO3-  = [d]

What is the cell potential at 25oC for the concentration cell described by: Cu(s) | Cu2+(aq, 0.10 M) || Cu2+(aq, 1.75 M) | Cu(s)

For a certain reaction at 330 K, ∆Hsys = -9.9 kJ and ∆Ssys = -85 J/K, calculate ∆Suniv.

Calculate ΔG°rxn for the following reaction at 298 K. NaCl(s) → NaCl(aq) ΔH° = 3.8 kJ;  ΔS° = 43.0 J/K Answer: ΔG°rxn  = [a] kJ

Calculate the molar solubility of M2X (Ksp = 1.3 x 10-21) in pure water. M2X(s) ⇌ 2M+(aq) + X2-(aq)

Consider a reaction that has a negative ΔH and a positive ΔS. Which of the following statements is true?  

Determine the standard entropy change (∆So) for this reaction. 3A2(g) ⟶2A3(g) Substance (state) So (J/mol.K) A(g) 150 A2(g) 200 A3(g) 250

Consider the following redox reaction in an acidic solution: I–(aq)  +  NO3-(aq)  → NO(g)  +  I2(s) When the equation is balanced with smallest whole number coefficients, the coefficient for — (a) NO  = [a] (b) NO3-  = [b] (c) H+  = [c] (d) H2O  = [d]

Calculate the mass of iron metal that will be deposited by passing a 85.0 A current through a solution of iron(II) chloride for 15.0 minutes. Fe2+(aq) + 2 e⁻  →  Fe(s)  You must show all of your work including units for credit.