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During the electrolysis of water , 4 molecules of electrons were transferred from anode to cathode the total volume of gases produced at the stp will be approximately?
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During the electrolysis of water , 4 molecules of electrons were trans...
Electrolysis of Water Overview
Electrolysis of water involves the decomposition of water (H₂O) into hydrogen (H₂) and oxygen (O₂) gases using electrical energy. The overall reaction can be summarized as:
\[ 2H₂O(l) \rightarrow 2H₂(g) + O₂(g) \]

Electrons Transferred
In this scenario, it is mentioned that 4 molecules of electrons were transferred. According to Faraday's laws of electrolysis, the number of moles of gas produced is directly related to the number of electrons transferred.

Understanding Gas Production
- **From the Reaction:**
- For every 4 electrons transferred, we can calculate the moles of gases produced.
- **Half-Reactions:**
- At the anode:
\[ 2H₂O \rightarrow O₂ + 4H^+ + 4e^- \]
- At the cathode:
\[ 4H^+ + 4e^- \rightarrow 2H₂ \]

Stoichiometry of Gases
- **Gas Moles Produced:**
- 4 electrons yield 1 molecule of O₂ (from 4e⁻ at the anode).
- 4 electrons yield 2 molecules of H₂ (from 4e⁻ at the cathode).
- **Total Volume Calculation:**
- Total gas produced = 2H₂ + 1O₂ = 3 moles of gas.

Volume at STP
- **Molar Volume at STP:**
- At standard temperature and pressure (STP), 1 mole of gas occupies approximately 22.4 liters.
- **Total Volume of Gases:**
- Total volume = 3 moles × 22.4 L/mole = 67.2 liters.
Thus, the total volume of gases produced during the electrolysis of water, when 4 molecules of electrons are transferred, will be approximately **67.2 liters** at STP.
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During the electrolysis of water , 4 molecules of electrons were transferred from anode to cathode the total volume of gases produced at the stp will be approximately?
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