How many moles of electrons are required to produce (a) 0.84 L of O2 at exactly 1 atm and 25C from aqueous H2SO4 solution; (b) 1.50 L of Cl2 at 750 mmHg and 20C from molten NaCl; (c) 6.0 g of Sn from molten SnCl2?

Problem 18.52How many moles of electrons are required to produce (a) 0.84 L of at exactly 1 atm and25C from aqueous solution; (b) 1.50 L of at 750 mmHg and 20C from moltenNaCl; (c) 6.0 g of Sn from molten Step by step solutionStep 1 of 3(a)0.84 L of at exactly 1 atm and 25C from aqueous solutionThe quantity of electricity carried by one mole of electrons is called a Faraday.Therefore, the number of moles of electrons which is equal to the number of faradays ofelectricity required.The overall cell reaction is as follows._______________________________________________________________Let’s calculate the number of moles of oxygen.Moles of a gas can be calculated by the ideal gas equation. ...................................(1)Rearrange the equation (1) ..................................(2)n = Number of moles of the gas\nP = pressureV = VolumeT = Temperature.From the given,Pressure = 1 atmVolume = 0.84 LGas constant = 0.0821 L.atm/mol. KTemperature = 298 KSubstitute the given values in the equation (2)Hence the number of produced moles of oxygen is 0.034 mol.Let’s calculate the number of faradays required to produce oxygen.From the cell reaction,One mole of oxygen produces four moles of electrons.The number of moles of electrons required to produce 0.034 moles of oxygen is calculated is asfollows.Let’s convert the 0.14 moles of electrons into faraday as follows.Therefore, 0.14 F required to produce 0.84 L of oxygen.___________________________________________________________________________