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