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Test02SOL-docAA

# 0 x 10 pa and t1 2405 k until the final 4 equilibrium

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Unformatted text preview: O(g) at 130. C and o 1.00 atm to a final state characterized by 1.30 mol H2O(l) at 30. C and 1.00 atm. The relevant constant o o pressure molar heat capacities are CPm (H2O(l)) = 75.3 J/K.mol and CPm (H2O(g)) = 33.6 J/K.mol. The initial state for the process described in Question 9 is identical to the initial state for the process described in Question 8. Similarly, the final state is the same for the processes described in Questions 8 and 9. Entropy is a state function; hence, its change is independent of the path as long as the same initial and final states are considered. So, ΔS for questions 8 and 9 must have the same value. Question 10: (10 points) 0.3177 g ethanol (C2H5OH(l)) is placed in an adiabatic constant volume bomb calorimeter of heat capacity, o - 1 CCAL = 8.80 kJ. C (this heat capacity accounts for both the calorimeter parts and the water in which the bomb is placed). Combustion of ethanol with an excess oxygen in the calorimeter at 298.15 K leads to formation of CO2(g) and H2O(l). Using the data in the thermodynamic table below, calculate the temperature change in the calorimeter. o Substance M (g/mol) ΔfH 298.15 K (kJ/mol) C2H5OH (l) - 267.69 46.07 CO2 (g) - 393.51 44.04 H2O (l) - 285.83 18.015 O2 (g) - - - 32.00 The combustion reaction for ethanol is written as: C2H5OH (l) + 3 O2 (g) à༎ 2 CO2 (g) + 3 H2O (l) The calorimeter equation is q = qCAL + qRXN = 0 since the calorimeter is adiabatic and the heat of reaction is transferred to...
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