if 9g of H20 is electrolysed completely with 50% current efficiency . calculate the amount of O2 (in Litres) formed at STP.
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M.M of H2O = 18g
Given Mass = 9g
mass of O2 in 18 g of H2O ---- 16g
mass of O2 in 1g of H2O ----- 1/16g
mass of O2 in 9g of H20 ------ 1/16*9*50/100
Given Mass = 9g
mass of O2 in 18 g of H2O ---- 16g
mass of O2 in 1g of H2O ----- 1/16g
mass of O2 in 9g of H20 ------ 1/16*9*50/100
tjjw13:
sorry by mistake
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Answer:
On complete electrlolysis of 9 g of Water we get 11.2/2= 5.6 Litres of oxygen at STP. It requires 1/2= 0.5 Faraday of electricity. Since the current efficiency is 50% , we require 2-times the amount of electricity. So we need= 0.5 x 2= 1 Faraday of electricity current, and liberates 5.6 Litres of Oxygen at STP.
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