Chem200HWChap5

Chem200HWChap5 - Chapter 5 1. a) Near room temperature, the...

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Chapter 5 1. a) Near room temperature, the specific heat capacity of ethanol is 2.42 J/ ° C.g. Calculate the heat needed to reduce the temperature of 150.0 g of C 2 H 5 OH from 50.0 ° C to 16.6 ° C. b) What mass of copper can be heated from 10 ° C to 200 ° C when 400 kJ of energy is available? The specific heat capacity of copper is 0.38 J/ ° C.g. 2. a) How much energy must be removed to lower the temperature of a 25.0 g block of ice (of specific heat capacity 2.03 J/ ° C.g ) from 12 ° C to –28 ° C? b) If the same energy were removed from 25.0 g of steam (of specific capacity 2.01 J/ ° C.g), what would be the temperature change? 3. A piece of metal of mass 20.0 g at 100 ° C is placed in a calorimeter containing 50.7 g of water at 22.0 ° C. The final temperature of the mixture is 25.7 ° C. What is the specific heat capacity of the metal? Assume that all the energy lost by the metal is gained by the water. 4.
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This note was uploaded on 09/09/2011 for the course CHEM 200 taught by Professor Saidane during the Spring '11 term at Mesa CC.

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Chem200HWChap5 - Chapter 5 1. a) Near room temperature, the...

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