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InterviewSolution
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Two electrolytic cells containing silver nitratesolution and dilute sulphuric acid wereconnected in a series. A steady current of 2.5 Awas passed through them till 1.078 g of silverwas deposited (Ag 107.8 g/mol)(a) How much electricity was consumed?(b) What is the weight of oxygen gas(i)liberated during the reaction? |
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Answer» Reaction :Ag^+ + e^- ----- Ag a. One mole of electrons are required to deposit one mole of silver (107.8 g/mol)= Charge of one mole of electrons = 96500 C= 96500 C ----- deposit 107.8 g of Ag= x C ----- deposit 1.078 gx = 96500 * 1.078 / 107.8 = 965 C of electricity is utilized. b. 2 H2O- ---- O2 + 4 H+ + 4e-= 96500 C ---- liberate 32 g of oxygen965 C liberate ----- 965 * 32 / 96500 = 0.32 g. b's answer is 0.16g |
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