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At constant volume, the heat of combustion of a particular compound is –3547.0 kJ/mol. When 1.239 g of this compound (molar mass = 196.58 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 8.539 °C. What is the heat capacity (calorimeter constant) of the calorimeter?

  • Chemistry -

    q = heat combustion
    q = heat capacity x delta T
    q = Cp x 8.539
    delta H = 3547.0 kJ/mol so
    q = 3547.0 kJ x (1.239/196.58) = ?
    Substitute and solve for Cp.

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