Calculate Electron Charge in 0.6 kg of Water

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To calculate the total electron charge in 0.6 kg of water, the mass is first converted to grams, resulting in 600 g. Dividing by the molar mass of water (18 g/mol) gives approximately 33.3 moles. Multiplying this by Avogadro's number yields about 2.01 x 10^25 molecules of water, and since each molecule contains 10 electrons, the total number of electrons is 2.01 x 10^26. Multiplying this by the charge of an electron (1.602 x 10^-19 C) results in a total charge of approximately 3.21 x 10^7 C. The calculation appears correct, but the answer may be rejected due to formatting or input errors in the online homework system.
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You have 0.6 kg of water. One mole of water has a mass of 18 g/mol and each molecule of water contains 10 electrons since water is H2O. What is the total electron charge contained in this volume of water? Answer in units for C.

First I converted 0.6 kg to 600 g. Then I divided that by 18 to get the number of moles, which was 33.3. Then I multiplied it by Avogadro's number to get the number of molecules and got 2.01 x 10^25. Then I multiplied it by the number of electrons, and got 2.01 x 10^26. Finally, I multiplied it by the electon charge, 1.602 x 10^-19, and got 3.21 x 10^7. This isn't right.
Am I going about this in the right way?
 
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it seems fine to me.. why do you think it's wrong?
 
It's an online homework problem, and when I typed in the answer it said it was wrong... I have no idea why though... I don't know any other way to do it.
 

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