Calculate the volume in cm3 of oxygen evolved as s.t.p. when a current of 5 A is passed through acidified water for 193s {F = 96500 Cmol-1, Molar volume of ...

Calculate the volume in cm3 of oxygen evolved as s.t.p. when a current of 5 A is passed through acidified water for 193s

{F = 96500 Cmol-1, Molar volume of a gas at s.t.p. = 22.4 dm3}

Answer Details

According to Faraday's laws of electrolysis, the mass of a substance produced at an electrode during electrolysis is directly proportional to the amount of electric charge passed through the cell. The relationship can be expressed as: mass of substance produced = (electric charge passed x molar mass of substance) / (Faraday's constant x charge on one electron) We can rearrange this equation to find the volume of gas produced at STP, as follows: volume of gas produced at STP = (electric charge passed x molar volume of gas at STP) / (Faraday's constant x charge on one electron) Substituting the given values into the equation, we get: volume of gas produced at STP = (5 A x 193 s x 22.4 dm3) / (96500 Cmol-1 x 1.602 x 10-19 C) Simplifying this expression, we get: volume of gas produced at STP = 0.056 dm3 Therefore, the volume of oxygen evolved as STP when a current of 5 A is passed through acidified water for 193 s is 0.056 dm3, or 56.000 cm3. The correct answer is.