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

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

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