3B.8 What is the change in entropy when (a) 100 g of iceis melted at 0 °C, (b) 100 g of water is heated from 0 °C to100 °C, and (c) 100 g of water is vaporized at 100 °C? Usethe values for each step to calculate the change in entropywhen 100 g of ice is converted into water vapour at 100 °C.Suppose that the changes are brought about by a heater thatsupplies energy at a constant rate. Sketch a graph showing(a) the change in temperature of the system, (b) the enthalpyof the system, (c) the entropy of the system as a functionof time.

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Answered: 3B.8 What is the change in entropy when…

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...

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Calculate the change in entropy (J/mol·K) for the surroundings for a reaction where ΔH° = 126.9 kJ/mol at 39.3°C. Report your answer to the tenths place and do not include units.
Calculate the change in entropy resulting from mixing the following gases (1 mole of A gas + 3 mole of B gas ) when the temperature is constant, knowing that R = 8.314 J / K. mol
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.
The entropy change for the processH2O(s)⟶H2O(l)is 27.9 J/K and requires that the surroundings transfer 35.0 kJ of heat to the system. Calculate the change in entropy for the universe in kJ/K at 56.2 °C.
Estimate the change in the entropy of the universe due to heat escaping from your home on a cold winter day.
The heat of fusion ΔHf of dichloromethane (CH2Cl2) is 6.2 kJ/mol. Calculate the change in entropy ΔS when 434.g of dichloromethane freezes at −95.1°C Be sure your answer contains a unit symbol and the correct number of significant digits.
For silicon, Si, the heat of fusion at its normal melting point of 1410 °C is 46.4 kJ/mol. The entropy change when 2.12 moles of liquid Si freezes at 1410 °C, 1 atm is J/K.
Which of the following processes will result in an increase in entropy for the system? (A) 2N2O(g) + O2(g) --> 4NO(g); (B) 2NO(g) + O2(g) --> 2NO2(g); (C) CO(g) + NO2(g) --> CO2(g) + NO(g); (D) SO3(g) + H2O(l) --> H2SO4(aq)
AG (ky/mol) SUbStance / 1on so (ky/mol) -1206.9 /moi k) 92.9 • CaC03l>) -|128.8 • CaO (s) |- 635. I – 60 3.5 38.2 • CO2(9) - 393.5 - 394.4 213.7 191.5 3 H2(g) 202.7 ZNH3 ) -45.9 -16 193 • Hz (g) 202.7 223.0 -92.31 - 95. 30 186.79
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.
Enter your answer in the provided box. Determine the change in entropy (ASys), for the expansion of 0.600 mole of an ideal gas from 2.00 L to 3.00 L at constant temperature. J/K < Prev 4 of 20 Nex
A mouse loses 36 J of heat per second. Calculate the change in entropy, ΔS, in J K–1, over the course of an hour at 27 °C. Take 0 °C = 273 K and state your answer to three significant figures and do not state units in the answer. ( please type answer not write by hend )

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