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. 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

Calculate the standard molar entropy of vaporization of water at 40.0 °C, given that its standard molar entropy of vaporization at 100.0 °C is 109.0 J-K-¹ mol and the molar heat capacities at constant pressure for liquid water and water vapor are 75.3 J-K-¹-mol-¹ and 33.6 J-K-¹-mol-¹, respectively, in this temperature range. A.Svap 145.96 Incorrect J.K-¹.mol-¹

The normal boiling point of ethanol is 78.3˚C, and its molar enthalpy of vaporization is39.3 kJmol-1(a) What is the change in entropy upon vaporization of ethanol at its boiling point?