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.

For the titration of 15.0 mL of 0.400 M HCl with 0.200 M NaOH. HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) a) What is the initial pH? pH =  b) What is the pH after the addition of 5.00 mL of NaOH ? pH =  c) What is the pH after the addition of 30.0 mL of NaOH? pH =  d) What is the pH after the addition of 35.0 mL of NaOH? pH =