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When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution...

When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter.

In the laboratory a general chemistry student finds that when 0.68 g of KOH(s) are dissolved in 104.30 g of water, the temperature of the solution increases from 22.14 to 23.80 °C.

The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.82 J/°C.

Based on the student's observation, calculate the enthalpy of dissolution of KOH(s) in kJ/mol.

Assume the specific heat of the solution is equal to the specific heat of water.

dHdissolution = ___kJ/mol

When I type the answer, will it have to be negative?

Solutions

Expert Solution

q   = -(q water + q calorimeter)

     = -(mcT + Ccal * T)

      = -(104.3*4.184*(23.8-22.14) + 1.82*(23.8-22.14))

      =- (724.409392 + 3.0212)

      = -727.43J

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

                               = 0.68/56   = 0.01214 moles

H = -q = -727.43J

                 = -727.43J/0.01214mole

                  = -59920J/mole

                   = -59.920KJ/mole >>>>answer

queen_honey_blossom answered 1 year ago
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