At 298 K , ∆H = 179.2 kJ and ∆S = 160.2 J/K for the reaction shown below. CaCO3(s)  ⟶ CaO(s) + CO2(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?

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

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. (b) What is the temperature above which the reaction is spontaneous?

Determine the balanced redox reaction represented by the following cell notation. Cu(s) ∣ Cu2+(aq) ∣∣ Zn2+(aq) ∣ Zn(s)

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+  = (b) Br-  = (c) Pb2+  = (d) BrO3-  =

Calculate the cell potential of a voltaic cell, which consists of a Sn/Sn2+ half-cell and a Zn/Zn2+ half-cell. Sn2+ + 2 e⁻  →  Sn Eo = -0.14 V Zn2+ + 2 e⁻  →  Zn Eo = -0.76 V

Consider the following redox reaction in acidic solution: HAsO2(s)  +  Cl2 (aq) → Cl- (aq)  +  H3AsO4(aq) When the equation is balanced with smallest whole number coefficients, the coefficient for — (a) HAsO2  = (b) Cl2  = (c) Cl-  = (d) H3AsO4  =

Use the standard free energies of formation (∆Gof) data to calculate the equilibrium constant for the reaction at 298 K. 2AB(g) ⇌ A2(g) + B2(g) Substance (state) ∆Gof (kJ/mol) A2(g) 0 B2(g) 0 AB(g) -10.0

Which of the following sets of compounds, when dissolved in the same solution, form a buffer solution?

Write the cell notation based on the description of the following voltaic cell: Silver ions are reduced to silver metal, and copper metal is oxidized to Cu2+ under standard conditions. Show your work including the two half-reactions.