When aq AgNO₃ is electrolysed using Pt electrodes, if 3.2 g of O₂ is liberated at the anode, the amount Ag that will be deposited at the cathode in grams is (at wt. of Ag = 108)

32 g

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1.6 g

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4.32 g

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43.2 g

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Solution

The correct option is D
43.2 g

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When aqueous $A g N O_{3}$ is electrolyzed using Pt electrodes, if 3.2 g of $O_{2}$ is liberated at the anode, the Amount of Ag that will be deposited at the cathode in grams is (at wt. of Ag = 108)

When aq. AgNO₃ is electrolysed using Pt electrodes if 3.2 g of O₂ is liberated at the anode, the amount Ag that will be deposited at the cathode in grams is (at wt. of Ag = 108)

Q. How many grams of silver would be deposited at cathode if

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of oxygen measured at NTP is liberated at the anode when silver nitrate solution is electrolysed between platinum electrodes?
(Given: Atomic mass of

A g = 108, O = 16

)

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is electrolysed between platinum electrodes, the substances liberated at anode and cathode are:

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of oxygen measured at NTP is liberated at the anode when silver nitrate solution is electrolyzed between platinum electrodes?(Given : Atomic masses of Ag = 108, O =16)

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When aq AgNO3 is electrolysed using Pt electrodes, if 3.2 g of O2 is liberated at the anode, the amount Ag that will be deposited at the cathode in grams is (at wt. of Ag = 108)

The correct option is D 43.2 g

When aq AgNO₃ is electrolysed using Pt electrodes, if 3.2 g of O₂ is liberated at the anode, the amount Ag that will be deposited at the cathode in grams is (at wt. of Ag = 108)

The correct option is D
43.2 g