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A 50.0 ml sample of a 1.00M solution if CuSO4 is mixed w/50.0 ml of 2.00...

A 50.0 ml sample of a 1.00M solution if CuSO4 is mixed w/50.0 ml of 2.00 Michelle KOH in a calorimeter. The temperature of both solutions was 20.2°C after mixing The heat capacity of the calorimeter is 12.1J/K. from these data calculate deltaH for the process.

CuSO4 (1M) +2KOH (2M) --> Cu (OH)2 +K2SO4(0.5M)

assume that the specific heat and density of the solution after mixing are the same as those of pure water and that the volumes are additive.

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Answer #1

   q   = mCT

    total mass of solution = 50 + 50 = 100ml

                                       = volume * density

                                         = 100*1 = 100g

q   = mCT

      = 100*4.18*(26.3-20.2)

      = 2549.8J

q = C*T

    = 12.1*(26.3-20.2) = 73.81J

q   = q1 + q2 = 2549.8+73.81 = 2623.61J

0.05 moles of K2So4 = 2623.61/0.05 = 52472.2J/mole = 52.4722KJ/mole

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