3. (2) Does the entropy of the surroundings always increase for spontaneous processes? Explain. (b) In a particular spontaneous process the entropy of the system decreases. What can you conclude about the sign and magnitude of ASur? (c) During a certain reversible process, the surroundings undergo an entropy change, - 75J/K. What is the entropy change of the system for this process?

3. (2) Does the entropy of the surroundings always increase for spontaneous processes? Explain. (b) In a particular spontaneous process the entropy of the system decreases. What can you conclude about the sign and magnitude of ASur? (c) During a certain reversible process, the surroundings undergo an entropy change, - 75J/K. What is the entropy change of the system for this process?

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

23. When a liquid changes to a gas, the entropy of the system (a) increases. (b) decreases. (c) remains the same. (d) the change in entropy cannot be predicted.
Does the entropy of the surroundings increase for spontaneous processes?
Explain in molecular terms why the entropy of a gas increases (a) with volume, (b) with temperature.
Calculate the change of the entropy of the system in J/K for the following phase transition: condensation of 64.1 g methanol The molar mass of methanol (CH3OH) is 32.04 g/mo%; the enthalpy of vaporization of methanol is 37.6 kJ/mol; the boiling point of methanol is 64.7°C A) -3640 B) -1130 C) 1.13446677 D) -223 E) 0.22258
Methanol is relatively inexpensive to produce. Much consideration has been given to using it as a precursor to other fuels such as methane, which could be obtained by the decomposition of the alcohol. CH3OH(l) -> CH4(g) + 1/2 O2(g) (a) What are the sign and magnitude of the entropy change for the reaction? Does the sign of Δ
(a) Does the entropy of the surroundings increase for spontaneousprocesses? (b) In a particular spontaneous processthe entropy of the system decreases. What can you concludeabout the sign and magnitude of ΔSsurr? (c) Duringa certain reversible process, the surroundings undergo anentropy change, ΔSsurr = -78 J/K. What is the entropychange of the system for this process?
ences to access important values if needed for this question. When 5.42 g of potassium bromide (KBr) is dissolved in 114g of water in a styrofoam calorimeter of negligible heat capacity, the temperature drops from 25.00 to 23.03 °C. Based on this observation, calculate q for the water and AH° for the process, assuming that the heat absorbed by the salt is negligible, KBr(s) K*(aq) + Br (aq) The specific heat of water is 4.184] °C¹g¹. Give the answers in kJ. ан, о AHO
A reaction has AH = -112 kJ and ASan = 354 J/K. At what temperature is the change in entropy for the reaction equal to the change in entropy for the surroundings?
Consider entropy and its role in determining if chemical and physical processes are spontaneous. For any process to be spontaneous, what must happen to the entropy of the universe during that process? Acetone will spontaneously vaporize when coming in contact with your skin even though acetone has a much higher boiling point. Explain how this occurs in light of your answer to part (a).
An endothermic reaction proceeds spontaneously. What can you deduce about the sign of Delta S for this process? Explain.
If AH = -70.0 kJ and AS = -0.300 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature. %3D Express your answer numerically in kelvins.