# Answer to Question #55972 in General Chemistry for tracy guido

Question #55972

You add 100.0g of water at 55.0C to 100.0g of ice at 0.00C. Some of the ice melts and cools the water to 0.00C. When thermal equilibrium is established at 0.00C, what mass of ice has melted?

Delta H of fusion for water is 333 J/g.

My question is I got a negative for q. Would this change to a positive because you need heat to melt the ice? I no you can't have a negative. So i am not sure if it should be a neg or a positive

q = m x specific heat x (Tfinal - Tinitial)

specific heat of water is 4.186 ( should memorize or on a chart)

q= 100g x 4.186J x ( 0 -55) = -23,023 J

mass ice x heat of fusion

q= m x Hfusion

-23,023J = m X 333 J/g = 69.12g

Delta H of fusion for water is 333 J/g.

My question is I got a negative for q. Would this change to a positive because you need heat to melt the ice? I no you can't have a negative. So i am not sure if it should be a neg or a positive

q = m x specific heat x (Tfinal - Tinitial)

specific heat of water is 4.186 ( should memorize or on a chart)

q= 100g x 4.186J x ( 0 -55) = -23,023 J

mass ice x heat of fusion

q= m x Hfusion

-23,023J = m X 333 J/g = 69.12g

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