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At constant volume, the heat of combustion of a particular compound is –3209.0 kJ/mol. When 1.829 g of this compound (molar mass = 159.29 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.753 °C. What is the heat capacity (calorimeter constant) of the calorimeter?

  • chem -

    How much heat was evolved in the combustion? That's 3209.0 kJ/mol x (1.829/159.29) = q = ?
    Then q = Ccal*delta T.
    Solve for Ccal.

  • chem -

    first you do n=m/M to get your moles then use you moles and the -3209.0 to geyt your kj then solve for the heat capacity by using the equation q=mct to rearrange to c=q/mt

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