What is ΔSsys for a boiling phase transition at 105.5 °C for a compound that boils at 105.5 °C and the ΔHsys = 69.9 kJ mol-1 for this process? Express your answer in J mol-1 K-1.
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What is ΔSsys for a boiling phase transition at 105.5 °C for a compound that boils...
What is ΔSsys for a freezing phase transition at 32.7 °C for a compound that freezes at 32.7 °C and the ΔHsys = -14.37 kJ mol-1 for this process? Express your answer in J mol-1 K-1.
What is ΔSsys for a freezing phase transition at 55.5 °C for a compound that freezes at 55.5 °C and the ΔHsys = -13.71 kJ mol-1 for this process? Express your answer in J mol-1 K-1.
What is ΔSsys for a melting phase transition at 10.2 °C for a compound that melts at 10.2 °C and the ΔHsys = 5.98 kJ mol-1 for this process?
What is ΔSsys for a condensation phase transition at 40.6 °C for a compound that condenses at 40.6 °C and the ΔHsys = -88.1 kJ mol-1 for this process?
What is the ΔSuniv for the following reaction at 25°C? N2(g) + 3H2(g) ⇌ 2NH3(g) ΔSsys = -197 J/K; ΔHsys = -91.8 kJ PLEASE SHOW WORK
Consider the data in the table. Compound Melting point (°C) AHfus (kJ/mol) Boiling point (°C) AH ap (kJ/mol) HF -83.11 4.577 19.54 25.18 НСІ -114.3 1.991 -84.9 17.53 HBr - 86.96 2.406 -67.0 19.27 HI -50.91 2.871 -35.38 21.16 Using the data in the table, calculate ASfus and ASvap for HI. ASfus = J/(K.mol) AS vap = J/(K · mol) Determine the entropy change when 6.50 mol HI(1) boils at atmospheric pressure. AS = J/K
What is ΔHsys for a reaction at 16.2 °C with ΔSsurr = 389 J mol-1 K-1 ? Express your answer in kJ mol-1 .
The fluorocarbon compound C2Cl3F3 has a normal boiling point of 47.6 ∘C. The specific heats of C2Cl3F3(l) and C2Cl3F3(g) are 0.91 J/g⋅K and 0.67 J/g⋅K, respectively. The heat of vaporization for the compound is 27.49 kJ/mol. Calculate the heat required to convert 45.5 g of C2Cl3F3 from a liquid at 14.10 ∘C to a gas at 78.40 ∘C. Express your answer using two significant figures.
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 J/g⋅K are 2.3 J/g⋅K respectively. A) How much heat is required to convert 30.5 g of ethanol at 30 ∘C to the vapor phase at 78 ∘C? Q=______kJ B)How much heat is required to convert 30.5 g of ethanol at -167 ∘C...
196 The normal boiling point of Br2(l) is 58.8 ∘C, and its molar enthalpy of vaporization is ΔHvap = 29.6 kJ/mol. a) When Br2(l) boils at its normal boiling point, does its entropy increase or decrease? b) Calculate the value of ΔS when 1.50 mol of Br2(l) is vaporized at 58.8 ∘C. ΔS= (answer in J/K)