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When 2.25mg of anthracene was combusted in a constant volume bomb calorimeter, the temperature rose by...

When 2.25mg of anthracene was combusted in a constant volume bomb calorimeter, the temperature rose by 1.35K. Given that the standard molar enthalpy of combustion of anthracene at 298K is -7061 kJ/mol, calculate the heat capacity of the calorimeter.

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Answer #1

    -7061KJ/mole   = -7061000J/mole

molar mass of anthracene   = 178.2g/mole

no of moles of anthracene    = W/G.M.Wt

   = 2.25*10^-3g/178.2g/mole    = 1.26*10^-5moles

= 7061000J/mole*.126*10^-5 mole

=      88.96J

q = mCT

88.96 = 0.00225*C*1.35

C    = 88.96/0.00225*1.35           = 29287.24J/g-K               

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