In calories.
heat lost by 16.2 g steam @ 100 C to condense to liquid is
q1 = mass x heat condensation.
q1 = 16.2 x 540 cal/g = ?
q2 = heat lost with H2O liquid moving from 100 C to 0C.
q2 = mass H2O x specific heat x (Tfinal-Tinitial) =
16.2 g x 1 cal/g*C x 100 C = ?
Total heat lost = q1 + q2 = ?
It takes 80 calories/g to melt ice so 80 cal/g x #g = q1 + q2
Solve for #g ice
How many grams of ice would be melted by the energy obtained as 16.2 of steam is condensed at 100 degrees celsius and cooled to 0 degrees celsius?
I would like to know how it's done step by step.
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