Solve Electrolysis Equation: 11.2L of Oxygen at STP

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The discussion centers on solving an electrolysis problem involving the production of oxygen from water. The key steps outlined for solving the problem include writing the balanced chemical equation for the electrolysis of water, determining the mole ratio of electrons transferred to the oxygen produced, and calculating the number of moles of electrons based on the given volume of oxygen (11.2L at STP). The next step involves converting the moles of electrons into charge measured in coulombs. Additionally, the application of Faraday's Law is suggested as a method to relate the charge transferred to the time taken when a specific current (0.5A) is applied. The overall goal is to clarify the calculations needed to find the required charge and the duration of the electrolysis process.
RPN
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hello
I saw someone had posted a question about this question but I too do not have a clear understanding of how to solve this equation. I have a very small section in my text about electroylsis and I have looked for information in others texts but I still need help. Please if anyone has an idea can you go through it step by step for me.
The question reads:
By the electrolysis of water, 11.2L of oxygen at STP was prepared
a) What charge was required?
b) If a current of 0.5A was used, how long did it take?
thank you
 
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Follow the standard steps :
1. Write the balanced eqn
2. Determine the mole ratio of electrons transferred to oxygen produced
3. From the given volume of oxygen determine the number of moles of electrons
4. Convert moles of electrons to charge in coulombs

OR

Balance and use Faraday's Law

From the charge transferred, the time taken at some current can be found
 

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