The molar heat capacities for carbon dioxide at 298.0 K are shown below. C 28.95 J K-¹ mol-1 C₂ = 37.27 J K ¹ mol-1 The molar entropy of carbon dioxide gas at 298.0 K and 1.000 atm is 213.64 J K-1 mol-¹. (a) Calculate the energy required to change the temperature of 1.000 mole of carbon dioxide gas from 298.0 K to 345.0 K, both at constant volume and at constant pressure. constant volume KJ kJ constant pressure (b) Calculate the molar entropy of CO₂(g) at 345.0 K and 1.000 atm. JK-1 mol-1 (c) Calculate the molar entropy of CO₂(g) at 345.0 K and 1.179 atm. JK-1 mol-1

The molar heat capacities for carbon dioxide at 298.0 K are shown below. C 28.95 J K-¹ mol-1 C₂ = 37.27 J K ¹ mol-1 The molar entropy of carbon dioxide gas at 298.0 K and 1.000 atm is 213.64 J K-1 mol-¹. (a) Calculate the energy required to change the temperature of 1.000 mole of carbon dioxide gas from 298.0 K to 345.0 K, both at constant volume and at constant pressure. constant volume KJ kJ constant pressure (b) Calculate the molar entropy of CO₂(g) at 345.0 K and 1.000 atm. JK-1 mol-1 (c) Calculate the molar entropy of CO₂(g) at 345.0 K and 1.179 atm. JK-1 mol-1

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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The molar heat capacities for carbon dioxide at 298.0 K are shown below. C₁ = 28.95 J K-¹ mol-1 C₂ = 37.27 J K-¹ mol-1 The molar entropy of carbon dioxide gas at 298.0 K and 1.000 atm is 213.64 J K-1 mol-1. (a) Calculate the energy required to change the temperature of 1.000 mole of carbon dioxide gas from 298.0 K to 340.0 K, both at constant volume and at constant pressure. constant volume kJ kJ constant pressure (b) Calculate the molar entropy of CO₂(g) at 340.0 K and 1.000 atm. JK-1 mol-1 (c) Calculate the molar entropy of CO₂(g) at 340.0 K and 1.201 atm. JK-¹ mol-1
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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 °℃
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