Faraday law of electrolysis Calculation worksheet 2023

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1 Faraday’s Law Of Electrolysis Calculations Worksheet Involving metals only 1 How many moles of copper are deposited when 5.0 A of current is passed through a solution of copper sulfate for 2 hours? 2 What is the mass of aluminum deposited when a current of 2.5 A is passed through an aluminum chloride solution for 10 minutes? 3 Calculate the time required to deposit 2.8 g of silver from a silver nitrate solution using a current of 0.50 A. 4 A current of 0.75 A is passed through a molten lead chloride for 1 hour. How many grams of lead are produced? Volume Or Mass Of A Gas 5 . What volume of oxygen gas is produced at STP when a current of 2.5 A is passed through water for 30 minutes? 6 A current of 0.40 A is passed through a solution of sodium sulfate for 20 minutes. Calculate the mass of hydrogen gas produced 7 How many grams of chlorine gas are produced when a current of 2.0 A is passed through a solution of hydrochloric acid for 1 hour 8 An electric current of 100 ampere is passed through a molten liquid of sodium chloride for 5 hours. Calculate the volume of chlorine gas liberated at the electrode at STP. 9 What current is required to produce 400.0 L of hydrogen gas, measured at STP, from the electrolysis of water in 1 hour (3600 s)? 10 Calculate the volume of chorine produced when a current of 2 A is passed though sodium chloride solution for 5 hours 40 minutes. Take the molar volume of a gas to be 23.8 l mol-1.ANS 50.31 litres 11 In the industrial production of chlorine gas, a current of 50,000 A was passed through a salt solution for 1 hour. Calculate the volume of gas which would be produced. Take the molar volume to be 24 dm 3 / mol 12 . Calculate the mass of hydrogen formed when a current of 0.4 A is passed through hydrochloric acid solution for 3 hours. ANS 0.045 g

2 13 A 40.0 amp current flowed through molten iron(III) chloride for 10.0 hours (36,000 s). Determine the mass of iron and the volume of chlorine gas (measured at 25 o C and 1 atm) that is produced during this time.. 14 An electric current of 100 ampere is passed through a molten liquid of sodium chloride for 5 hours. Calculate the volume of chlorine gas liberated at the electrode at NTP. 15 What current strength in ampere will be required to liberate 10 g of chlorine from sodium chloride solution in one hour? [125.09 second ] In Series Calculation 16 In an electrolysis experiment, a current was passed for 5 hours through two cells connected in series. The first cell contains a solution gold salt and the second cell contains copper sulphate solution. 9.85 g of gold was deposited in the first cell. If the oxidation number of gold is +3, find the amount of copper deposited on the cathode in the second cell. Also calculate the magnitude of the current in ampere. [0.0804 ampere] 17 An electric current of 100 ampere is passed through a molten liquid of sodium chloride for 5 hours. Calculate the volume of chlorine gas liberated at the electrode at NTP. 18 During the electrolysis of concentrated copper(ll)chloride solution using carbon electrodes, 3.2 g of copper was deposited at the cathode. Calculate the volume of chlorine gas evolved at the anode at s.t.p. 19 What mass of silver is deposited from silvertrioxnitrate (v) solution at the same time as 2.40 g of copper from copper(ll) tetrasulphate(VI) solutions are arranged in series connected to a battery?. 20 find the volume of oxygen evolved at the anode at the same time as 3.2 of Cu is deposited on the cathode when copper II tetraoxosulphate (VI) solution is electrolysed between platium electrodes Agalvanic cell is up under standard conditions unsing Aluminium and Nickel electrodes as shown in the diagram below

3 After the cell has been operating for a period of time, the gain in mass at the nickel cathodes is 1,77g. 21.1 Calculate the number of moles of Nickel which have been deposited at the cathode. 2 21.2 Calculate the subsequent loss in mass at the Aluminium Anode 3 NORTH WEST 2015 22.The diagram represents galvanic cell (A). A small light bulb connected in the external circuit glows brighly. 22.1 If 0.4 moles of electrons flow to the the cathode,What will be the decrease in mass of the Anode?

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4 23. The diagram below represents a galvanic cell that works under standard conditions. (Olivier O A) The Cell is allowed to discharge for a period, duringwhich the mass of the copper elctrode changes by 3.2 g. Calculate the expected change in the mass of the silvernelectrode.(Accept that the change in mass is only due to the oxidation- reductionthat takesplace as the cell discharges)

5 PAST PAPERS Faraday’s law of electrolysis worksheet Ieb 2022

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7 MEMO

8 Nov 2021 MEMO

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