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.

Calculate ∆Go for the following reaction at 298 K. CH3OH(g)  ⇌ CO(g) + 2H2(aq)    Kc = 7.1 x 10-6

Which substance in the given pairs has the higher entropy value ? a) HNO3(aq) or b) HNO3(l) a) C2H5OH(l) or b) C3H7OH(l) a) HCl(g) or b) HBr(g)

1. Select the strongest acid from the following: A) HClO or HClO2 B) HI or HBr 2. Select the strongest base from the following: C) NO2- or NO3- 3. Which will be more soluble in an acidic solution? D) CuCO3 or CuBr2

Which of the following acids is the weakest? The acid is followed by its Ka value.