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    combustion of quinone

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    1)When a 9.55 g- sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter, the temperature rises from 23.6 C to 47.4 C .
    Calculate the molar enthalpy (in kJ/mol NaOH) for the solution process NaOH(s)>>Na+(aq)+OH-(aq) . Assume that the specific heat of the solution is the same as that of pure water.

    2)A 2.300 g sample of quinone (C6H4O2) is burned in a bomb calorimeter whose total heat capacity is 7.854 kJ/C. The temperature of the calorimeter increases from 23.90C to 31.35C.
    - What is the heat of combustion per gram of quinone?
    - What is the heat of combustion per mole of quinone?

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    https://brainmass.com/chemistry/energetics-and-thermodynamics/combustion-of-quinone-308303

    Solution Preview

    1) We need to assume that the heat yielded by dissovling NaOH is absorbed by the solution.
    so first calculate the heat absorbed by the solution:
    Q = mc * deltaT.
    where the mass of the solution = 9.55 + 100.0 = 109.55 grams.
    the specific heat of pure water c = 4.184 J/(g.K)
    the temperature change ...

    Solution Summary

    It shows how to calculate the molar enthalpy during hydroxide dissolving process. It also calculates the heat from the combustion of quinone.

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