(1/2)Zn2+(aq) + e- → (1/2) Zn(s) In the reaction above, calculate the quantity of electricity required to discharge zinc. [F = 96 500 C mol-1]

The quantity of electricity required to discharge zinc can be calculated using Faraday's law, which states that one mole of electrons carries a charge of 96,500 Coulombs. The given chemical equation shows that the reduction of 1 mole of Zn2+ requires the gain of 2 electrons (1/2 Zn2+ + e- → 1/2 Zn). Therefore, to discharge 1 mole of Zn2+, 2 moles of electrons are needed. Using Faraday's law, we can calculate the quantity of electricity required to discharge 1 mole of Zn2+: 1 mole of Zn2+ requires 2 * 96,500 C = 193,000 C Therefore, to calculate the quantity of electricity required to discharge zinc from the given half-reaction, we need to divide 193,000 C by 2 (since the reaction involves half-moles of Zn2+): Quantity of electricity required = 193,000 C / 2 = 96,500 C Comparing this value with the options given, we can see that the correct answer is: 9.650 * 104 C This matches the value of Faraday's constant, which was given in the question.