______________________ accelerates the rusting process.

A concentration cell has the same half-reactions at the anode and cathode, but a voltage results from different concentrations in the two electrode compartments.(b) A similar cell has 0.10 M Cu2+ in both compartments. When a stoichiometric amount of ethylenediamine (NH2CH2CH2NH2) is added to one compartment, the measured cell potential is 0.179 V. Calculate the formation constant Kf for the complex ion Cu(NH2CH2CH2CH2)22+. Assume there is no volume change.

Consider the redox titration of 100.0 mL of a solution of 0.010 M Fe2+ in 1.50 M H2SO4 with a 0.010 M solution of KMnO4, yielding Fe3+ and Mn2+. The titration is carried out in an electrochemical cell equipped with a platinum electrode and a calomel reference electrode consisting of an Hg2Cl2/Hg electrode in contract with a saturated KCl solution having [Cl-] = 2.9M. Using any data in Appendixes C and D, calculate the cell potential after addition of (a) 5.0 mL, (b) 10.0mL, (c) 19.0 mL, and (d) 21.0 mL of the KMnO4 solution.

Using the Nernst equation, calculate the concentration of Cu^2+ ions given the cell potential is 0.5540 V and the standard cell potential is 0.4260 V. The equation is: 0.5540 V = 0.4260 V - (0.0592/2) log ([Cu^2+]/[1]^2). What is the concentration of Cu^2+?

A voltaic cell is constructed with two Zn2+-Zn electrodes, where the half-reaction is Zn2+ + 2e- → Zn(s) with E° = -0.763 V. The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10^-2 M, respectively. What is the cell emf in volts?

At 25°C, E° = +1.88 V for a cell based on the reaction 3 AgCl(s) + Al(s) → 3 Ag(s) + Al³⁺(aq) + 3 Cl⁻(aq). Find the cell potential E if [Al³⁺] = 0.20 M and [Cl⁻] = 0.010 M using the Nernst equation.

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Cu(s) | Cu2+(aq, 3.2×10^(-3) mol L^-1) || Cu2+(aq, 4.48 mol L^-1) | Cu(s). Given E°(Cu2+/Cu) = +0.34 V, express your answer to two significant figures.