A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a galvanic cell constructed with a graphite electrode and a half-cell of AgCl(s) + e⁻ → Ag(s) + Cl⁻(aq) E°red = 0.2223 V And a copper electrode with 0.500 M Cu²⁺ as the second half cell Cu²⁺(aq) + 2 e⁻ → Cu(s) E°red= 0.337 V The measured cell potential when the water sample was placed into the silver side of the cell was 0.0687 V. What is the standard cell potential for this cell in V?

Consider a galvanic electrochemical cell constructed using Cr/Cr³⁺ and Zn/Zn²⁺ at 25 °C. The following half-reactions are provided for each metal: Cr³⁺(aq) + 3 e⁻ → Cr(s) E°red = -0.744 V Zn²⁺(aq) + 2 e⁻ → Zn(s) E°red = -0.763 V Given that the standard cell potential is 0.019 V and the overall equation is 2 Cr³⁺ (aq) + 3 Zn (s) → 2 Cr (s) + 3 Zn²⁺ (aq), what is the cell potential for this cell at 25 °C when [Zn²⁺] = 0.0323 M and [Cr³⁺] = 0.1736 M?

Consider the following reaction and its AG° at 25.00 °C. Fe2+(aq) + Zn(s) – Fe(s) + Zn?+(aq) AG° = -60.73 kJ/mol Calculate the standard cell potential, Eel» for the reaction. E V 'cell Calculate the equilibrium constant, K, for the reaction. K =

What is the cell potential for a voltaic cell having one electrode composed of a Zn strip dipped in a 0.034 M Zn(NO)(aq) solution and the other electrode composed of a Zn strip dipped into a 0.414 M Zn(NO)(aq) solution? Assume all other cell components are in place and the temperature is 25.0°C.   To produce 1.21 kg of solid potassium from molten KCl, how many hours must 0.721 amps be passed through the KCl?   How many hours will you have to electrolyze the forks to apply 0.500 g of Ag to each one? Your electrolysis device operates at a current of 3.75 amps.