The mass of silver (Molar mass of Ag : 108 gmol–1 ) displaced by a quantity of electricity which displaces 5600 mL of O2 at S.T.P. will be _____ g.
Correct Answer: 108
Solution and Explanation
To determine the mass of silver (Ag) displaced by the quantity of electricity that liberates 5600 mL of O2 at standard temperature and pressure (STP), we first calculate the moles of O2. At STP, 1 mole of any gas occupies 22.4 L (22,400 mL). Therefore, the moles of O2 are:
Moles of O2 = \(\frac{5600 \,\text{mL}}{22400 \,\text{mL/mol}} = 0.25 \,\text{mol}\)
The electrolysis of water produces O2 according to the reaction: 2H2O → 4H+ + O2 + 4e-. This indicates that 4 faradays of electricity are required to produce 1 mole of O2.
Consequently, 0.25 moles of O2 require:
0.25 × 4 = 1 faraday of electricity
The reduction of silver ions to silver metal is represented by: Ag+ + e- → Ag. This reaction shows that 1 faraday of electricity deposits 1 mole of Ag.
Given that the molar mass of Ag is 108 g/mol, 1 faraday of electricity will deposit:
108 g of Ag
Thus, the mass of silver displaced is 108 g.
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