Help me Completed 4 out of 900 010ResourcesSubmit AllQuestion 6 ofGeneral Chemistry 4th EditionMcQuarrie Rock GalloglyUniversity Science Bookspresented by Macmillan LearningPredict how the entropy of the substance is affected in cach process.0,(r. 200 kPa, 300 K) 0,(r. 100 kPa, 300 K)entropyL(g. I bar, 125 "C) L(E. I bar, 200 "C)entropyH,O(g, 75 Torr, 300 K) H,O(g. 150 Torr, 300 K)entropy50

Here we have to predict in the following processes in which entropy increase or decrease.

Versity Science Books presented by Macmilan Learning MEOUame Rock Galogly Predict how the entropy of the substance is affected in each process 0,tr, 200 kPa, 300 K) 0,(r. 100 kPa, 300 K) entropy 1,(r. 1 bar, 125 "C) L(e. 1 har, 200 "C) entropy H,O(g, 75 Torr, 300 K) H,0(e, 150 Torr, 300 K) entropy

Versity Science Books presented by Macmilan Learning MEOUame Rock Galogly Predict how the entropy of the substance is affected in each process 0,tr, 200 kPa, 300 K) 0,(r. 100 kPa, 300 K) entropy 1,(r. 1 bar, 125 "C) L(e. 1 har, 200 "C) entropy H,O(g, 75 Torr, 300 K) H,0(e, 150 Torr, 300 K) entropy

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter10: Energy

Section: Chapter Questions

Problem 18ALQ

See similar textbooks

Similar questions

At 298K, NH4NO3 readily dissolves in water, suggesting that the change in free energy (ΔG) favors the dissolution process. However, when NH4NO3 dissolves in water, the temperature of the water decreases. The particulate diagram above attempts to provide a microscopic view of the dissolution of NH4NO3(s) considering both the change in enthalpy (ΔH) and the change in entropy (ΔS). Which of the following explains what the particle diagram is able to illustrate and why? (see attached image) a.) The particle diagram is able to illustrate that the ΔH for the dissolution of NH4NO3 is exothermic because overcoming the attractive forces between the ions requires the absorption of energy. b.) The particle diagram is able to illustrate that the ΔH for the dissolution of NH4NO3 is endothermic because forming new interactions between the ions and the water molecules releases energy. c.) The particle diagram is able to illustrate that entropy increases when NH4NO3(s) dissolves in water…
Please help answer unanswered parts: Calculations 1 and 2 (at bottom, red boxes) Equation used was as follows: C [crystal graphite] + CO2 [gas ] ⇌ 2CO [gas ] ; Formation of carbon monoxide Equation: C [crystal graphite] + CO2 [gas] + <---> 2CO [gas] + + Standard Enthalpy of Formation and Entropy ∆fHo(T) (KJ/mol) So(T) (J/mol.K) C [crystal graphite] 18.51 30.32 CO2 [gas] -343.41 283.87 CO [gas] -78.69 243.42
Use the calibration curve data provided to determine the entropy (ΔS, in J/K) associated with dissolving KNO3. please put the answer in this format: ____x10___power ___units *use correct sig figs
Assume that solutions of ethylbenzene : benzene behave ideally. a) Calculate the entropy of mixing if 40 g of ethylbenzene is mixed into 50 g of benzene.b) At room temperature (298 K), what is ΔmixG for mixing 40 g of ethylbenzene (PhEt) and 50 g of benzene (PhH)?c) Would you notice a temperature change associated with the process in parts a) & b)?d) Instead you mix 40 g of benzyl alcohol (PhMeOH) into 50 g of benzene (PhH). Let’s denote the difference between this process and the process in part b) as:ΔΔG = ΔmixG[ PhMeOH ∶ PhH ] − ΔmixG[ PhEt ∶ PhH ]What do you expect the sign of ΔΔG to be? ( ΔΔG < 0, ΔΔG ≈ 0, or ΔΔG > 0 )Briefly justify your answer.
The Mond process relies on the volatility of Ni(CO)4 for its success. Underroom conditions, this compound is a liquid, but it boils at 42.2°C with anenthalpy of vaporization of 29.0 kJ mol-1 . Calculate the entropy of vaporization of Ni(CO)4, and compare it with that predicted by Trouton’s rule.
Assume that solutions of ethylbenzene : benzene behave ideally. a) Calculate the entropy of mixing if 40 g of ethylbenzene is mixed into 50g of benzene.b) At room temperature (298 K), what is ΔmixG for mixing 40g of ethylbenzene (PhEt) and 50g of benzene (PhH)?c) Would you notice a temperature change associated with the process in parts a) & b)?d) Instead, you mix 40g of benzyl alcohol (PhMeOH) into 50g of benzene (PhH). Let’s denote the difference between this process and the process in part b) as: ΔΔG = ΔmixG [PhMeOH ∶ PhH] − ΔmixG [PhEt ∶ PhH] What do you expect the sign of ΔΔG to be? (ΔΔG<0, ΔΔG≈0, or ΔΔG>0)Briefly justify your answer.
A system goes from state 1 to state 2 and back to state 1. (a) Is ∆E the same in magnitude for both the forward and reverse processes?
If the change of entropy of the surrounding increased by 0.27 KJ/mol.K due t oa reactiob carried out at a 25C tempreture ,which one of these following terms apply to the reaction?cricle all the correct answers. Exergonic endergonic exothermic endothermic
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 chart is prepared by plotting In Ksp versus 1/T, using data obtained by performing a lab experiment. Refer to the attached photo for guidance on how to perform these calculations; Equation 5 is particularly useful. A linear fit of the data in the chart yields the equation y = (-4.976x10^3)x+(1.9900x10^1) with an R2 value of 0.9922. Determine the entropy (deltaS in J/K) associated with dissolving KNO3. Answer in scientific notation with appropriate sigfigs.
10. The thermodynamic functions for the generic reaction A+B=>C at 25oC are: ΔH=-35.7 kJ/mole; ΔS=-6.95 J/mole*K Calculate ΔG in kJ/mole Group of answer choices 146 -37.7 -35.5 -33.6 2036
Two students prepared aqueous solutions of LiCl and measured the properties, as shown in the table above. Both students observed that the solid LiCl readily dissolved in H2O. The students drew particle diagrams to explain the changes in the enthalpy and entropy of dissolution for LiCl based on their results and observations. Based on this information, the better particle diagram was drawn by which student, and why is that diagram more accurate? (see attached image) a.) The better particle diagram was drawn by Student 1 because when LiCl dissolves in water, it dissociates into Li+ and Cl− ions causing an increase in entropy. b.) The better particle diagram was drawn by Student 1 because when LiCl dissolves in water, it dissociates into Li+and Cl−ions indicating that the dissolution of LiCl is exothermic. c.) The better particle diagram was drawn by Student 2 because it shows that LiCl does not dissociate, resulting in a decrease in entropy for the dissolution of LiCl.…