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A 1.55 gram sample of methanol (CH3OH) is combusted in a bomb calorimeter. The molar heat of combustion of methanol is -725KJ/mole, assuming that 2.0L of water initially at 25.0 C absorbs all of the heat of combustion, what is the final temperature of the water?

  • chemistry -

    2CH3OH + 3O2 ==> 2CO2 + 4H2O
    How many heat is emitted by 1.55 g CH3OH? That will be
    725 kJ x (1.55 g/(2*molar mass CH3OH) kJ. Change that to J, then
    J = mass H2O x specific heat H2O x (Tfinal-25). Solve for Tf. I think the answer is close to 27 C.

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