Whenever a gas expands when we exhale, when a flask is opened, and so on thegas undergoes an increase in entropy. Conversely, when a gas contracts, its entropydecreases.(a) Show that the entropy change đue to reversible isothermal expansion orcontraction of a perfect gas is AS = nR In(V¼V;), where V; and V; are the initialand final volumes, respectively.(b) Calculate the change in molar entropy when carbon dioxide expandsisothermally from 1.5 L to 4.5 L.(c) A sample of carbon dioxide that initially occupies 15.0 L at 250 K and 1.00atm is compressed isothermally. Into what volume must the gas be compressedto reduce its entropy by 10.0 JK-

Answered: Image /qna-images/answer/24fd9dc9-c988-4f5c-a67e-28ec1546906c.jpg

Whenever a gas expands when we exhale, when a flask is opened, and so on the gas undergoes an increase in entropy. Conversely, when a gas contracts, its entropy decreases. (a) Show that the entropy change due to reversible isothermal expansion or contraction of a perfect gas is AS = nR In(VV), where V, and V½ are the initial and final volumes, respectively. (b) Calculate the change in molar entropy when carbon dioxide expands isothermally from 1.5 L to 4.5 L. (c) A sample of carbon dioxide that initially occupies 15.0 L at 250 K and 1.00 atm is compressed isothermally. Into what volume must the gas be compressed to reduce its entropy by 10.0 JK-

Whenever a gas expands when we exhale, when a flask is opened, and so on the gas undergoes an increase in entropy. Conversely, when a gas contracts, its entropy decreases. (a) Show that the entropy change due to reversible isothermal expansion or contraction of a perfect gas is AS = nR In(VV), where V, and V½ are the initial and final volumes, respectively. (b) Calculate the change in molar entropy when carbon dioxide expands isothermally from 1.5 L to 4.5 L. (c) A sample of carbon dioxide that initially occupies 15.0 L at 250 K and 1.00 atm is compressed isothermally. Into what volume must the gas be compressed to reduce its entropy by 10.0 JK-

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

(b) Further predict the sign of change in entropy with proper explanation for the following cases. (i) Isothermal expansion of a perfect gas (ii) Cleaning the room with a vacuum cleaner
Determine the entropy of * 2H2(g) + O2(g) → 2H₂O(1) positive negative
Use the data from this table of thermodynamic properties to calculate the maximum amount of work that can be obtained from the combustion of 1.00 mole of ethane, CH3CH3(g), at 25 °C and standard conditions. mo
Calculate the change in entropy for a sample heated from 298 K to 500 K under constant pressure. The constant pressure heat capacity is 29 J/mol K.
A2 Calculate the change in molar entropy of trichloromethane when heated from 0.00C to 270C. The constant pressure molar heat capacity fits the expression 91.47 + 7.5 × 10-2(T/K) between 240 K and 330 K.
Ice cubes at 0°C are poured into a glass that initially contains 150 g of liquid water at 20°C. The contents of the glass are gently stirred. After a short time, some of the ice melts, and the liquid cools to 0°C. No appreciable heat exchange occurs between matter inside the glass with matter outside the glass during this process. (a) Calculate the entropy change of the universe during the process. Use only the following data: the constant pressure heat capacity of liquid water is approximately 4.18 J/(g K) over the temper- ature range of interest. You may further presume that the density of water is constant over the temperature range. (b) If the same process were performed reversibly, how much useful work would be obtained from it? Any required heat exchange to achieve the same final state reversibly should be with matter outside the glass, which are at 20°C.
Estimate the change in the entropy of the universe due to heat escaping from your home on a cold winter day.
Calculate the molar entropy of a constant-volume sample of argon at 270 K given that it is 154.84 J K–1 mol–1 at 298 K. Unit in J/mol-K.
Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction entropy of the following chemical reaction: Al,03 (s)+ 3H, (g) → 2Al (s) + 3H,O (g) Round your answer to zero decimal places. x10 K
quantity (iv) Why is the universe regarded A4. Define Gibb's free energy. Show that the Gibb's free energy change of a system at constant temperature is given by AG=AH-TAS pings
(c) [5 pts] Sketch a graph of the entropy of the van der Waals gas and the entropy of the perfect gas as a function of Vm for b = 1. What happens as b→ 0? Take n = 1 and plot S/nR. (d) [5 pts] Explain the intuition for the graph in (c) using the Boltzmann entropy and the number of microstates.
The enthalpy of vaporization (deltaHvap) of water was experimentally determined to be 151.3 kJ for 3.72 mols of water at 100 degrees Celsius? Calculate the molar entropy of vaporaization (deltaSvap,m) of water.