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.

1.00 mol SO3 is placed in a 1.00 L vessel at 425 K and allowed to come to equilibrium at which time 0.250 mol SO3 remains. 2SO3(g) ⇌ 2SO2(g) + O2(g) A) Calculate the equilibrium concentration of SO2(g) [a] mol/L B) Calculate the equilibrium concentration of O2(g) [b] mol/L C) Calculate KC [c] D) Calculate KP [d]

Calculate ΔSsurr at 298 K. 2NO2(g) → N2(g) + 2O2(g) ΔH = -66.4 kJ

A chemical equilibrium may be established by starting a reaction with ___________________

Determine the Kb for CN- at 25°C. The Ka for HCN is 4.9 × 10-10.

1. Select the strongest acid from the following: A) HNO3 or HNO2 [a] B) HCl or HBr [b] 2. Select the strongest base from the following: C) ClO- or ClO2- [c] 3. Which will be more soluble in an acidic solution? D) PbCl2 or PbF2 [d]

For the reaction A + 3B → 2C, how does the rate of disappearance of B compare to the rate of production of C?

Calculate the pH of a solution that contains 3.9 × 10-5 M H3O+ at 25°C.

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

For the titration of 15.0 mL of 0.200 M HCl with 0.200 M NaOH. HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) a) What is the initial pH? pH =  [a] b) What is the pH after the addition of 5.00 mL of NaOH ? pH =  [b] c) What is the pH after the addition of 15.0 mL of NaOH? pH =  [c] d) What is the pH after the addition of 20.0 mL of NaOH? pH =  [d]