The heat of vaporization of water at the normal boiling point, 373.2 K, is 40.66 kJ/mol. The specific heat capacity of liquid water is 4.184 JK-1g-1 and of gaseous water is 2.02 J K-1g-1. Assume that these values are independent of temperature. What is the heat of vaporization of water at 298.2 K? Does this result agree with Appendix 4 data?
Answer to relevant QuestionsConsider the following reaction at 248oC and 1.00 atm: CH3Cl(g) + H2(g) → CH4(g) + HCl(g) For this reaction, the enthalpy change at 248oC is 283.3 kJ/ mol. At constant pressure the molar heat capacities (Cp) for the ...You have a 1.00-mole sample of water at 230oC, and you heat it until you have gaseous water at 140.oC. Calculate q for the entire process. Use the following data: Specific heat capacity of ice = 2.03 JoC-1g-1 Specific heat ...For nitrogen gas the values of Cv and Cp at 25oC are 20.8 J K-1 mol-1 and 29.1 J K-1 mol-1, respectively. When a sample of nitrogen is heated at constant pres-sure, what fraction of the energy is used to increase the ...A sample of ice weighing 18.02 g, initially at 230.0oC, is heated to 140.0oC at a constant pressure of 1.00 atm. Calculate q, w, ΔE, ΔH, and ΔS for this process. The molar heat capacities (Cp) for solid, liquid, and ...Predict the sign of ΔSo for each of the following changes. a. b. AgCl(s) → Ag+(aq) + Cl-(aq) c. 2H2(g) + O2(g) → 2H2O(l) d. Na(s) + 1/2 Cl2(g) → NaCl(s) e. HCl(g) → H+(aq) + Cl2(aq) f. KBr(s) → K+(aq) + Br-(aq)
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