For each system listed in the first column of the table below, decide (ifpossible) whether the change described in the second column willincrease the entropy s of the system, decrease s, or leave s unchanged.If you don't have enough information to decide, check the "not enoughinformation" button in the last column.olaSystemChangeASO As < 0O AS = 0The water condenses to a liquid at aA few grams of water vapor (H20).constant temperature of 3.0 °C.O As > 0not enoughinformationO As < 0The carbon dioxide is cooled fromO As = 062.0 °C to -1.0 °C and is alsoA few moles of carbon dioxide (CO2) gas.expanded from a volume of 3.0 L toa volume of 4.0 L.O As > 0not enoughinformationO AS< 0The helium is cooled from 26.0 °C toO As = 0A few moles of helium (He) gas.-13.0 °C while the volume is heldconstant at 2.0 L.O As > 0not enoughinformation

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy s of the system, decrease s, or leave s unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System Change AS O As<0 O AS = 0 A few grams of water vapor (H,0). The water condenses to a liquid at a constant temperature of 3.0 °C. O As>0 not enough information O As<0 The carbon dioxide is cooled from O AS = 0 62.0 °C to -1.0 °C and is also A few moles of carbon dioxide (CO.) gas. expanded from a volume of 3.0 L to O As>0 a volume of 4.0 L. not enough information O AS<0 The helium is cooled from 26.0 °C to O AS = 0 A few moles of helium (He) gas. -13.0 °C while the volume is held constant at 2.0 L. O As > 0 not enough information O O o O

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy s of the system, decrease s, or leave s unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System Change AS O As<0 O AS = 0 A few grams of water vapor (H,0). The water condenses to a liquid at a constant temperature of 3.0 °C. O As>0 not enough information O As<0 The carbon dioxide is cooled from O AS = 0 62.0 °C to -1.0 °C and is also A few moles of carbon dioxide (CO.) gas. expanded from a volume of 3.0 L to O As>0 a volume of 4.0 L. not enough information O AS<0 The helium is cooled from 26.0 °C to O AS = 0 A few moles of helium (He) gas. -13.0 °C while the volume is held constant at 2.0 L. O As > 0 not enough information O O o O

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter16: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 1ALQ: For the process A(l) A(g), which direction is favored by changes in energy probability? Positional...

See similar textbooks

Similar questions

For the process A(l) A(g), which direction is favored by changes in energy probability? Positional probability? Explain your answers. If you wanted to favor the process as written, would you raise or lower the temperature of the system? Explain.
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)
For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column.
For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. Note for advanced students: you may assume ideal gas and ideal solution behaviour.
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.
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
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
What will be the Gibbs free energy in KJ/mol if the entropy of the reaction (ΔS°rxn) is 301.59 KJ/mole and the ethlapy (ΔH°rxn) is -394.59 J/mol at 27.73 oC? Answers in 2 decimal place , unit is not required.
A xenon gas sample at at initial temperature, volume and pressure of 20C, 20dm3 and 2 atm, repectivley, expands to a final pressure of 1 atm, while being heated to 80C. Calculate the change in entropy of this process
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.
1 mol super cooled liquid water transformed to solid ice at -10 oC under 1 atm pressure. Calculate entropy change of the system, surrounding and universe. (temperature of the environment is -10 °C) Please use the following data for water : Melting entalpy of ice (ΔHmelting) at 0°C and 1 bar is 6020 J mol-1. Cp (H2O (s)) = 37,7 J mol-1 K-1 Cp (H2O (l)) = 75,3 J mol-1 K-1
For the complete neutralization reaction between a 1 M strong acid and a 1 M strong base of equal initial volumes that is marked by a temperature rise, the entropy of neutralization is positive (ΔSrxn > 0) whereas the Gibbs free energy is negative (ΔGrxn < 0). Is this true or false? Please explain.