Write anode and cathode reactions from electrolysis of water. How much charge will be transported for the decomposition of 3.6 g of H₂O? [F = 96500 C mol^–1]

Solution

At cathode: $4 H^{+} + 4 e^{-} \to 2 H_{2} (g)$
At anode: $2 H_{2} O \to O_{2} + 4 H^{+} + 4 e^{-}$

36 g of $H_{2} O$ requires $4 \times 96500 C$

3.6 of $H_{2} O requires \frac{4 \times 96500}{36} \times 3.6 = 38600 C .$

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Electrochemistry

Write anode and cathode reactions from electrolysis of water. How much charge will be transported for the decomposition of 3.6 g of H₂O? [F = 96500 C mol^–1]

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Electrochemistry

Write anode and cathode reactions from electrolysis of water. How much charge will be transported for the decomposition of 3.6 g of H2O? [F = 96500 C mol–1]

Some More Questions From Electrochemistry Chapter

If the current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons flow through the wire?

Suggest a list of metals that are extracted electrolytically.

Consider the reaction: Cr2O72– + 14H+ + 6e- → 2Cr3+ + 8H2OWhat is the quantity of electricity in coulombs needed to reduce 1 mol of Cr2O72-?

Write the chemistry of recharging the lead storage battery, highlighting all the materials that are involved during recharging.

Suggest two materials other than hydrogen that can be used as fuels in fuel cells.

Name the electrolyte used in fuel cell?

Can we use copper vessel to store AgNO3 solution ?

Suggest a metal that can be used for cathodic protection of iron against rusting.

Mock Test Series

NCERT Sample Papers

Entrance Exams Preparation

Write anode and cathode reactions from electrolysis of water. How much charge will be transported for the decomposition of 3.6 g of H₂O? [F = 96500 C mol^–1]

Consider the reaction: Cr₂O₇^2– + 14H⁺ + 6e- → 2Cr³⁺ + 8H₂O
What is the quantity of electricity in coulombs needed to reduce 1 mol of Cr₂O₇^2-?

Can we use copper vessel to store AgNO₃solution ?