For the ΔG° values given here, determine the standard cell potential for the cell.(a) 12 kJ/mol, n = 3(b) −45 kJ/mol, n = 1

How long (in hours) must a current of 5.0 amperes be maintained to electroplate 60g of calcium from molten CaCl2?

An electrochemical cell consists of a half-cell in which a piece of platinum wire is dipped into a solution that is 2.5 M in KI and 0.046 M in I2. The other half-cell consists of magnesium metal immersed in a 0.37 M Mg2+ solution. Assume that the temperature is 25°C. (a) Which electrode is the anode and which is the cathode? anode: Pt|I2, I- O Mg²+|Mg cathode: O Pt|I2, I- Mg2+|Mg (b) What is the emf of the cell? 4.0 2.869 X V (c) What is the spontaneous cell reaction? chemPad OHelp Greek - Mg2+(aq)+21 (aq) Mg(s)+I2(aq) Mg(s)+l_2(aq)-->Mg^2+(aq)+2l^-(aq) Your answer appears to have inconsistent states-of-matter. (d) What is the equilibrium constant of the cell reaction? 2.42e98