Chemistry 12

The molar heat of vaporization of water is 42 kJ/mol. How much energy is released by the condensation of 3.0 g of water?

So for water there will just be one mol.
I think this is how you do it, but it doesn't match the answer in the worksheet.

q=mc delta t
But we're not given a temperature?
q= (3.0g)(4.18 J/g x degrees celsius)
q= 12.54

And we know that + or - q= Hrxn

And that Hrxn=Hvap
???
I think I'm not even on the right track. Any help would be really appreciated. Thank you!!!

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  1. You're right. You started out wrong.
    q = mols H2O x heat condensation
    mols H2O = grams/molar mass = 3/18 = ?
    q = (3/18) x 42,000 J = ? J released.

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