In an electrolysis cell similar to the one employed In this experiment. a student observed at his unknown metal anode lost 0.233 g while a total volume of 94.50 mL of H ₂ was being produced. The temperature in the laboratory was 25?C and the barometric pressure was 740 mm Hg. At 25?C the vapor pressure of water is 23.8 mm Hg. To find the equivalent man hie metal, he filled in the blanks below. Fill In the blanks as he did.

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PH, Phar-VPH₂0 T=K ₂ - mL. moles 1 mole H₂ requires passage of. No. of faradays passed Loss of mass of metal anode - MM Cu " mm Hg = PV RT liters No. grams of metal lost per faraday passed - faradays no. grams lost no. faradays passed The student was told that his metal anode was made of copper. g. The charge n on the Cu ion is therefore atm - g = EM (Eq. 3) PH, Phar-VPH₂0 T=K ₂ - mL. moles 1 mole H₂ requires passage of. No. of faradays passed Loss of mass of metal anode - MM Cu " mm Hg = PV RT liters No. grams of metal lost per faraday passed - faradays no. grams lost no. faradays passed The student was told that his metal anode was made of copper. g. The charge n on the Cu ion is therefore atm - g = EM (Eq. 3)

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Explanation 1 PH 2 P bav VP H20 740 mm Hg 238 mm Hg 7162 mm Hg 1 atm 760 mm Hg 2 1 ... View the full answer