Consider a simple galvanic cell consisting of two beakers connected by a salt bridge. One beaker contains a solution of MnO." in dilute sulfuric acid and has a Pt electrode. The other beaker contains a solution of Sn in dilute sulphuric acid, also with a Pt electrode. When the two electrodes are connected by a wire, current flows and a spontaneous reaction occurs that is described by the following balanced chemical equation: 2Mn0ja2) + 5Sn²* (aq) + 16H* (ag) → 2Mn²* (ag) + 5Sn** (aq) + 8H20u For this galvanic cell, a. Write the half – reaction that occurs at each electrode b. Indicate which electrode is the cathode and which is the anode c. Indicate which electrode is the positive electrode and which is the negative electrode

How many grams of Tungsten metal are plated out when a constant current of 13.00 A is passed through an aqueous solution containing W5+ ions for 527 minutes?

Determine the ΔG° in KJ for a voltaic cell made of a Ag strip and a Pb strip immersed in 1.0 M aqueous AgNO3 and Pb(NO3)2 solutions, respectively, with all other cell components in place. (Use Table 18.3 for your standard cell potentials.)   Determine the thermodynamic equilibrium constant K for a voltaic cell made of a Zn strip and a Pb strip immersed in 1.0 M aqueous Zn(NO3)2 and Pb(NO3)2 solutions, respectively, at 25.00°C, with all other cell components in place. (Use Table 18.3 for your standard cell potentials.)

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

A non-standard state galvanic cell is constructed at 25.00°C as described here.  The Fe(s) anode is immersed in a 0.040 M Fe(NO3)2 solution.  The Cu(s) cathode is immersed in a 0.0060 M Cu(NO3)2.  The circuit is completed with a salt bridge containing 1.0 M KNO3.  The standard Fe/Fe2+ reduction potential is –0.44 V.  The standard Cu/Cu2+ reduction potential is +0.34 V.  Calculate the non-standard-state cell potential for this galvanic cell and determine if the reaction described is spontaneous under these conditions.

Molten CaCl2 can be electrolyzed to form metallic Ca. For what duration should an electrolysis be performed at a current of 2.67 A in order to produce 15.1 g Ca?