Question:
A battery delivers a steady current of \(3.00\) ampere for \(10.0\) hours. Calculate the number of moles of electrons passed.
A battery delivers a steady current of \(3.00\) ampere for \(10.0\) hours. Calculate the number of moles of electrons passed.
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Find the total charge as current times time, then divide by the charge carried by one mole of electrons (the Faraday constant).
Updated On: Nov 12, 2026
- \(3.6\)
- \(1.12\)
- \(4.5\)
- \(2.7\)
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The Correct Option is B
Solution and Explanation
Step 1: Understanding the Concept
Charge passed is \(Q = I\times t\).
One mole of electrons carries one Faraday, \(F \approx 96500\text{ C}\).
Step 2: Calculation
\(t = 10.0\text{ h} = 10\times 3600 = 36000\text{ s}\)
\(Q = 3.00\times 36000 = 108000\text{ C}\)
Moles of electrons \(=\dfrac{108000}{96500}\approx 1.12\text{ mol}\)
Step 3: Compare the options
The value \(1.12\) matches the second option.
Final Answer:
About 1.12 moles of electrons are passed. \[ \boxed{\text{(B) }1.12} \]
Charge passed is \(Q = I\times t\).
One mole of electrons carries one Faraday, \(F \approx 96500\text{ C}\).
Step 2: Calculation
\(t = 10.0\text{ h} = 10\times 3600 = 36000\text{ s}\)
\(Q = 3.00\times 36000 = 108000\text{ C}\)
Moles of electrons \(=\dfrac{108000}{96500}\approx 1.12\text{ mol}\)
Step 3: Compare the options
The value \(1.12\) matches the second option.
Final Answer:
About 1.12 moles of electrons are passed. \[ \boxed{\text{(B) }1.12} \]
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