CuSO4(aq) + Mg(s) MgSO4(aq) + Cu(s) a) Write the net ionic equation. b) Write the two half-cell reactions. c) The equilibrium is favored to the right. Write the formula for the two oxidizing agents and circle the stronger one.

A certain half-reaction has a standard reduction potential -0 red = = +0.90 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 0.70 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. ロ→ロ 0 Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a minimum. ☐v red If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. no minimum Ś ? 0 Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a maximum. Ov red If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. no maximum E E = = X

Electrolytic process of determining molar mass.  An electrolysis cell contains X3+ ions. When a 5.45 A current is passed through the cell for 2.16 x 103 s, 8.50 g of elemental X are formed. What is the molar mass of X and at which electrode does X appear?

Please don't give handwritten answers   is the strongest oxidising agent under standard conditions? Ag+(aq) H2(g) H+(aq) Cl2(g) Al+3(aq)