Determination of an Equivalent Mass by Electrolysis In an electrolysis cell simi

Question

Determination of an Equivalent Mass by Electrolysis In an electrolysis cell similar to the one used in this experiment, a student reported that his unknown metal lost 0.2330 g while a total volume of 94 50 ml of H2 was being produced The temperature in the laboratory was 25.0 degree C and the barometric pressure was 740.0 mm Hg. At 25 0 degreeC the vapor pressure of water is 23.8 mm Hg Fill in the blanks below to determine the equivalent mass of the unknown metal. 1 mole H2 requires the passage of_____ moles of faradays Number of faradays passed = (2 n h2) Loss of mass of metal anode = _____ g No. of grams of metal lost / faraday passed = # grams lost / # faradays passed The student was told that the metal anode was copper The charge on the Cu ion is therefore

Explanation / Answer

Let us determine the number of moles of hydrogen produced on cathode.

PV = nRT,

So, n =number of moles = PV / RT.

P(H2) = P_bar - VP_H2O = 740 - 23.8 = 716 mm Hg = 0.942 atm.
V(H2) = 94.50 mL = 0.0945 L (given).
T = 25

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