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Unformatted text preview: of the water is 34.2 o C, what is the specific heat of the metal? 7. 75.0 g of ice are left in a cup on the counter and eventually melt. How much heat is required to melt the ice? The heat of fusion of water is 334 J/g. The heat of vaporization of water is 2.260 kJ/g. 8. Calculate the amount of heat you would need to convert 18.0 g of ice at -25 o C to steam at 125 o C. Heat of fusion of water = 334 J/g Heat of vaporization of water = 2.260 kJ/g Specific heat of ice = 2.03 J/g K Specific heat of water = 4.18 J/g K Specific heat of steam = 1.84 J/g K Key 1. 0.475 J/g o C or 0.114 cal/g o C 2. 24 cal 3. 3.02 kcal 4. 29.1 o C 5. 15.5 Calories 6. 0.831 J/g o C This one is challenging! Here are some hints to help. #1 The energy of the hot metal = the energy used to heat up the water. #2 The final temperature of the metal is the same as the final temperature of the water. 7. 25.0 kJ 8. 56.0 kJ (If you solve this, you can solve anything!)...
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This note was uploaded on 03/08/2012 for the course CHEM 101 taught by Professor Anderson,w during the Fall '08 term at BYU.
- Fall '08