Question

In the electrolysis experiment similar to the one employed in this experiment; a student observed that his unknown metal anode lost 0.238 grams while a total volume of 94.50 mL of hydrogen was being produced.

The temperature of the solution was 25 °C and the barometric pressure was 740 mm Hg.

The vapor pressure of water at 25 °C is 23.8 mm Hg.

1. What is the pressure of the hydrogen gas in atmospheres?

                                                                                                                

2. What is the volume of hydrogen gas in liters?

3. Calculate the number of moles of hydrogen gas using the ideal gas law (For checking yourself, the answer is between 0.003 and 0.004 moles)

4. One mole of H2 requires passage of ______ Faradays

5. Number of Faradays passed = ______________

6. EM = ____________________

7. The student was told the metal was oxidized to a +2 oxidation state. What is the metal in the anode?

Answer 1

gas , in atm Pns-ProtalPMo 20mm Hg - 23.8 mm 16.24 mina X lahn 76omm o.442 ahn Noo, volumuHyaron gas V L O 04SL Noo, Na the ideal Lauo, (0a42ahm)0.09us) RT 00821 Lalmmol29 - 3.64 X1o3 moles o Oo 36 molog M6lar mars anknon metal 0.230 modeg maN Motarmau 6s.39 mol Thi metar mas i having oxldatlon no, 2 a gtven n e quasron matal in tho 'anode Thus, the MSo, I mole t regruisee 2 molu elechonu =2 faraday used S4, th number savacday 2 Co.0036 O 00 728