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Nitrous oxide, N2O(g), reacts with carbon disulfide, CS2(g) according to the equation below. When performed in...

Nitrous oxide, N2O(g), reacts with carbon disulfide, CS2(g) according to the equation below. When performed in a constant volume bomb calorimeter with a heat capacity of 8.775 kJ °C–1 , the temperature of the calorimeter rises from 22.5 °C to 29.1 °C and forms 2.48 g of sulfur, S8. Determine the molar internal energy, ∆U, and the molar enthalpy, ∆H (both in kJ mol-1 ) of the following reaction at 25.0 °C.

3 N2O(g) + CS2(l) ® 3 N2(g) + CO(g) + 1/8 S8(s)

Solutions

Expert Solution


3 N2O(g) + CS2(l) ---> 3 N2(g) + CO(g) + 1/8 S8(s)

heat released(q) = C*DT

C = heat capacity of calorimeter = 8.775 kj /c

DT = 29.1-22.5 = 6.6 c

q = 8.775*6.6 = 57.9 kj

no of mol of S8 formed = w/Mwt

                       = 2.48/256

                       = 0.0097 mol

so hat, formation of 0.0097 mol S8 = 57.9 kj

        formation of 1/8 mol S8 = 57.9*(1/8)*(1/0.0097)

                                = 746.13 kj

DUrxn = -746.13 kj

Dn = nP-nR

   = 4-3

   = 1

DHrxn = DU+DnRT

Dn = 1 , R = 8.314*10^-3 kj.k-1.mol-1 , T = 25 c = 298 k

      = (-746.13)+1*8.314*10^-3*298

      = -743.6 kj

queen_honey_blossom answered 2 years ago
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