Question

#2

(a) For the combustion of 0.04 mol of C5H12O (l) at constant pressure and a temperature of 25.00oC, 170kJ of heat released by this reaction is measured. With this data, what are the values ​​of ΔH, ΔU, Q, and W for the combustion of 1,000 moles of C5H12O (l) at constant volume and a temperature of 25.00oC? Combustion is the reaction of a substance with O2 (g) to produce CO2 (g) and H2O (l).

(b) (3 points) We have an unknown liquid. For its vaporization, what are the signs (positive or negative) for its enthalpy variation, its entropy variation, and the variation in the entropy of the surroundings? You don't need to explain your answers.

Answer 1

Sof Since. Process is Constant volume & isothermed W-O-DV0 soo T=constont U-f() too ideas ges From Ist Low of Thermodynamics = Dua W O =DH + PDV+VDP +W TO=DH = 170 UI hence T s. inuessed (6) tre Foo repourischon DH ss tve DS suro -ve.

using given data and first law of thermodyanamics and ideal gas assumption we can find the required variables and signs

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