How much water is ionized in the lightning?

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The discussion focuses on calculating the amount of water ionized by lightning, questioning how many electrons are involved in this process. A mole of water weighs 18.1 g, and Avogadro's number is provided for conversion purposes. The initial calculation attempted to determine the number of water molecules ionized but resulted in incorrect units. Participants express uncertainty about the necessary information to accurately calculate the ionization and mention the need for the total charge in a lightning bolt. The conversation concludes with a humorous guess of 42 as the answer, highlighting the complexity of the question.
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If each water molecule donates one electron,
how much water is ionized in the lightning?
One mole of water has a mass of 18.1 g/mol.
Answer in units of g.


Avogadro’s number is 6.02214e23 /mol.


ok so this is what i did...
(18.1grams/1mole)(1mol/6.02214e23 molecules)=3.005576e-23
this is wrong since it doesn't give the right units. How would i do this?
 
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How many coulombs in that bolt of lightning and what fraction of those electrons are involved in the ionization of water.

Not enough information but I'm guessing the answer is 42.
 
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