Calculate the entropy of mixing at constant temperature and pressure for the mixing of two ideal gases in the molar ratio 3:2. The total moles of the two gases combined are 10 moles. Take the universal gas constant, R to be 8.3145 J mol k!. O A. -55.96 J/K B. -389.29 J/K C. 389.29 J/K D. 55.96 J/K E. 1354.91 J/K

Calculate the entropy of mixing at constant temperature and pressure for the mixing of two ideal gases in the molar ratio 3:2. The total moles of the two gases combined are 10 moles. Take the universal gas constant, R to be 8.3145 J mol k!. O A. -55.96 J/K B. -389.29 J/K C. 389.29 J/K D. 55.96 J/K E. 1354.91 J/K

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter13: Spontaneous Processes And Thermodynamic Equilibrium

Section: Chapter Questions

Problem 46AP

See similar textbooks

Similar questions

What is the temperature of the low-temperature reservoir of a process that has an efficiency of 0.440(44.0) and a high-temperature reservoir at 150C?
List the sets of conditions that allow dS, dU, and dH of a process in a system act as a spontaneity condition.
Why isnt the entropy of elements in their standard pressure at normal that is, room temperatures equal to zero?
What is the temperature of the high - temperature reservoir of a process that has an efficiency of 44.0(0.440) and a low - temperature reservoir at 150C?
Use equations 4.21 and 4.25 to explain why H and G vary much more with pressure for a gas than they do for a solid and a liquid.
A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it exerts pressure of 2000 psi. Calculate the work (in J) performed when this gas expands isothermally against an opposing pressure of 1.0 atm. (The amount of work that can be done is equivalent to the destructive force of about 1/4 lb of dynamite, giving you an idea of how potentially destructive compressed gas cylinders can be if improperly handled!)
The molar heat capacity for carbon monoxide at constant volume is ??, ?=20.17 J/(K·mol)CV, m=20.17 J/(K·mol). A 9.009.00-L fixed-volume flask contains CO(g) at a pressure of 9.009.00 kPa and a temperature of 25.0 °C. Assuming that carbon monoxide acts as an ideal gas and that its heat capacity is constant over the given temperature range, calculate the change in entropy for the gas when it is heated to 800.0 °C.
Benzene (C6H6) has a melting point of 5.50C and an enthalpy of fusion of 10.04kJmol-1 at 25.00C. The molar heat capacities at constant pressure for solid and liquid benzene are 100.4JK-1mol-1 and 133.0JK-1mol-1, respectively. Calculate the change of entropy of system and change of entropy of the surrounding at 100C for the reaction of C6H6(l)---->C6H6(s)
A certain monatomic substance has only one solid form, which melts at 190.2K and then remains liquid to above 298.2K. The heat of fusion is 5891 J/mol, and the average heat capacities of the solid and the liquid may be taken to be 35.6 and 53.1 J/mol-K, respectively. At 18K, the heat capacity was found to be 2 J/mol-K. Calculate the approximate third law entropy of this compound
1.00 mol each of Ne, Ar and Kr are kept in separate cylinders at a pressure of 1 bar and a temperature of 298 K. The cylinders are then connected and the three gases mix. Consider the gases as ideal. Calculate the absolute entropy of this system at OK.
Half a mole of a perfect gas expands isothermally and at 298.15 K from a volume of 10 L to avolume of 20 L. (a) What is the change in the entropy of the gas? (b) How much work is doneon the gas? (c) What is the heat of Surroundings ? (d) What is the change in the entropy of the surroundings? (e)What is the change in the entropy of the system plus the surroundings?
Calculate change in entropy of a system where 10.0 g of ice at -10.0 ° C is converted to water vapor at 115.0 ° C and a constant pressure of 1 bar. The heat capacity at constant pressure of H2O (s) and H2O (l); is 75.291 J / (K-1 mol-1); and of H2O (g); is 33.58J / (K-1 mol-1)