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Chemistry Problem Set: Heat Energy and Temperature

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The specific heat capacity of benzene is 1.74J/g*K. What is its molar heat capacity (Jmol*K)?

What quanity of heat is required to raise the temperature of 50.00mL of water from 25.52 to 28.75C? The density of water at this temperature is 0.997 g/mL.

When 108g of water at a temperature of 22.5C is mixed with 65.1g of water at an unknown twmperature, the final temperature of the resulting mixture is 47.9C. What was the initial temperature of the sample of water?

What quanity of heat energy (in joules) is required to raise the temperature of 454g of tin from room temperature (25.0C) to its melting point, 231.9C and then melt the tin at that temperature? The specific heat capacity of tin is 0.227 J/g*K, and the heat fusion of this metal is 59.2J/g.

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Solution Summary

Molar heat capacityBenzene = specific heat capacityBenzene * MolarMassBenzene
Heat = mass of water * specific heat of water * temperature difference
Heat of Sample1 = (-)Heat of Sample2
Total Heat = massTin * specific heat capacityTin* Temperature difference + Heat fusionTin* massTin

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The specific heat capacity of benzene is 1.74J/g*K. What is its molar heat capacity (Jmol*K)?

Molar heat capacityBenzene = specific heat capacityBenzene * MolarMassBenzene
= (1.74 J/g*K ) * ( 78 g/mol )
= 135.72 J/mol*K

What quanity of heat is required to raise the temperature of 50.00mL of water from 25.52 to ...

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