The vapor pressure of a liquid is 47.1 kPa at 501 K and 10.5 kPa at 489 K. What is the enthalpy of vaporization of the liquid ?

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  =