Consider the process below. The normal boiling point of CH3CN is 82 °C. CH;CN(g, 103 °C, 1 atm) CH3CN(I, 68 °C, 1 atm) You may assume that the temperature of the surroundings is constant and also equal to 68 °C. Which of the following statements about the process below is/are correct? Select all that apply. You may choose more than one, or none, of the statements. The entropy of the system increases: AS > 0. O The entropy of the surroundings increases: ASurr > 0. O The entropy of the universe increases: ASuniv> 0. O Work is done by the system on the surroundings. Heat flows from the system into the surroundings. O The process is thermodynamically irreversible.

Consider the process below. The normal boiling point of CH3CN is 82 °C. CH;CN(g, 103 °C, 1 atm) CH3CN(I, 68 °C, 1 atm) You may assume that the temperature of the surroundings is constant and also equal to 68 °C. Which of the following statements about the process below is/are correct? Select all that apply. You may choose more than one, or none, of the statements. The entropy of the system increases: AS > 0. O The entropy of the surroundings increases: ASurr > 0. O The entropy of the universe increases: ASuniv> 0. O Work is done by the system on the surroundings. Heat flows from the system into the surroundings. O The process is thermodynamically irreversible.

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

O ENTROPY AND FREE ENERGY Predicting qualitatively how entropy changes with temperature. OD 15 Nerbs V 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 not enough O information AS 0 not enough information O AS 0 not enough information Fxplanation Check 0 Terms of Use I Privacy Center| Accessibility O 2022 McGraw Hill LLC. All Rights Reserved. re to search 99+ IA
Consider the following reaction at 25 °C: 5 SO3(g) + 2 NH3(g) → 2 NO(g) + 5 SO2(g) + 3 H20(g) If AH° = 42.4 kJ./mol and AS° = 562.3 J/mol•K, estimate the temperature at which this reaction would be at equilibrium assuming that enthalpy and entropy are independent of temperature. %3D %3D
Three moles of N2(g), originally at 0.25 atm pressure, are mixed isothermally with 5 moles of H₂(g), also at 0.25 atm pressure, to yield a mixture whose total pressure is 0.025 atm. What is the molar entropy of mixing (in J mol-¹ K-¹)?
For each of the following reactions determine if the change in entropy was positive or negative:A) Water at 40°C → Water at 25°CB) 2NO2(g) → N2O4(g)C) CH3OH (l) → CH3OH (g)D) PbCl2(s) → PbCl2(aq)
By examining the following graphs, predict which element- copper or gold-has the higher absolute entropy at a tem- perature of 200 K. 0.3 0.2 Au Cu 0.1 100 200 300 Temperature (K) 7U mol-! K-2)
Calculate the equilibrium PCO₂ at 25°C for reaction below. Report your answer to three significant figures. CaCO3(s)CaO(s) + CO₂(g) x 10 atm (Enter your answer in scientific notation.) Standard Thermodynamic Values at 298 K Substance CaCO3(s) CaO(s) CO₂(g) CO,(aq) AGf (kJ/mol) -1,128.8 -603.5 -394.4 -386.2 Prev 20 of 25 ‒‒‒ ‒‒‒
1. Please consider 0.15 gm of Constantan (a Cu/Ni alloy widely used in thermocouples, c = 390 J/•K-kg) that cooled through exposure to the laboratory atmosphere (T 22 •C) from 620 C to 20 C. a. Please determine the change in entropy of the Constantan (in J/ K- kg). b. Please determine the change in entropy of the laboratory atmosphere (in J/ K-kg). c. Please determine the change in entropy of the universe (in J/ K-kg). %3D
Elemental carbon usually exists in one of two forms: graphite or diamond. It is generally believed that diamonds last forever. The table shows the standard enthalpy of formation (AH) and the standard molar entropy (Sº) values for diamond and graphite. Part A AGrxn= What is the standard Gibbs free energy for the transformation of diamond to graphite at 298 K? Cdiamond →Cgraphite Submit Express your answer to three significant figures and include the appropriate units. ► View Available Hint(s) O Substance Cgraphite Cdiamond μA Value AH (kJ/mol) Units 0 1.897 ? S° (J/mol. K) 5.740 2.38
5). Calculate the standard entropy change for the following two reactions. Consult the last page of the exam for data and equations. a) 2 CO(g) + O2(g) à 2 CO2(g) b) 2 NaHCO3(s) à Na2CO3(s) + H2O(l) + CO2(g)
1)spontaneous or non spontaneous 2) the change in Gibbs free energy is negative or the change in Gibbs free energy is positive 3)positive or negative
Place the following species in order of decreasing molar entropy at 55°C. Assume that they are all in the gas phase. SiO2 Si4H10 SiO SiO2 > Si4H10 > SiO Si4H10 > SiO2 > SiO SiO2 > SiO > Si4H10 SiO > Si4H10 > SiO2 Si4H10 > SiO > SiO2 SiO > SiO2 > Si4H10
The vaporization of compound A is described by the following chemical equation. AH (72.41 °C) = 40.89 kJ/mol A(1)→ A(g) Calculate the entropy of vaporization, A.Sap for A(1) at 25.0 °C given that the boiling point of A is 72.41 °C, and the molar heat capacity of A(1) is 114.59 J/(mol K). Assume that the molar heat capacity of A(g) is 56.3% of that of A(1). A.Svap = Calculate the standard enthalpy of vaporization, AHp, for A(1) at 25.0 °C. Allie Calculate the standard Gibbs free energy of vaporization, AG, at 25.0 °C. AG- Determine the equilibrium constant, K, for the vaporization at 165.0 °C. T= Is the vaporization of A(1) spontaneous at temperatures greater than or less than T? J. mol. K Determine the temperature at which the vaporization of A(1) becomes spontaneous. Assume that the enthalpy and entropy of vaporization change very little with temperature. O less than 7 Ogreater than 7 kJ/mol kJ/mol °℃