Question

3. If the amperage in your electrolysis cell were increased by a factor of 2, what effect would this have on the time required to produce the same amount of hydrogen? 4. Electrolysis of an NaCl solution with a current of 2.00 A for a period of 200 s produced 59.6 mL of Cl2 at 650 mm Hg pressure and 27 °C. Calculate the value of the Faraday's Constant from these data. 5. Why are different products obtained when molten NaCI and aqueous NaCl are electrolyzed? Predict the products in each case.

Answer 1

If amperage in your electrolysis cell were increased by a factor of 2, what effect would this have on the time required to produce the same amount of hydrogen rightarrow it will cut the time in half electrolysis of Nacl solution with current for a period of 200 s produced 59.6 m L of cl_2 at 650 mm Hg pressure and 27 degree c calculate the value of faradays constant moles of cl_2 p_1 v_1/T_1 = p_2 v_2/T_2 i.e, 650 times 59.6/300 k = 760 times v2/273 v2 = 56.015 m 1 mole of any gas at = 22.4 L standarg T and p 56.015 m_2 0.056015/22.4 = 0.0025 mol amount of electricity used = amp times sec = 2 times 200 = 400 coulombs to make 0.0025 mole of cl_2 = 400 coulomb 1 mole of cl_2 = 160000 coulomb cl^- ion 1 faraday to make 1 mole of