In an electrolytic cell similar to the one used in this experiment, a student collected 94.50 mL of hydrogen gas at a temperature of 25 C. The barometric pressure was 740 mmHg and the vapor pressure of water at 25 C is 23.8 mmHg. The unknown metal anode lost 0.233 g during the electrolysis.
a) Calculate the number of moles of hydrogen gas formed.
b) Calculate the number of moles of electrons (faradays) passed in the cell during the electrolysis.
c) Calculate the equivalent mass of the metal.
d) If the charge on the metallic cation is known to be 2+, calculate the molar (atomic) mass of the unknown metal. Use the periodic table to identify this metal.