A sample of ethanol (C₂H₅OH) was burned completely in a bomb calorimeter whose total heat capacity is 30.75 kJ/^oC. The temperature of the calorimeter plus the contents increased from 25.6^oC to 32.7^oC.

Knowing that ethanol's heat of combustion is -3330 kJ/mol, calculate the mass of the sample (in g).

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Sixta KovacekLv2

15 May 2019

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A 1.800-g sample of phenol (C₆H₅OH) was burned in a bomb calorimeter whose total heat capacity is 11.66 kJ/°C. The temperature of the calorimeter plus contents increased from 21.36 to 26.37 °C. (a) Write a balanced chemical equation for the bomb calorimeter reaction. (b) What is the heat of combustion per gram of phenol? Per mole of phenol?

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The heat capacity of a bomb calorimeter was determined by burning 6.73 g of methane (energy of combustion = −803 kJ/mol CH₄) in the bomb. The temperature changed by 12.0°C.

(a) What is the heat capacity of the bomb?

(b) A 14.4-g sample of ethanol (C₂H₅OH) produced a temperature increase of 13.8°C in the same calorimeter. What is the energy of combustion of ethanol (in kJ/mol)?