AH° = 301.5 kJ/mol, AS° = 761.4 J/mol-K %3D %3D Calculate the boiling point temperature (in K) at standard conditions,

Calculate the energy released as heat when 18.7 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. heat capacity of Hg(1) Constants for mercury at 1 atm melting point enthalpy of fusion 28.0 J/(mol-K) # 234.32 K 2.29 kJ/mol 9 = MacBook Pro

Can you help part A A metal salt with the formula MCI, crystallizes from water to form a solid with the composition MCI, • 6H2O. The equilibrium vapor pressure of water above this solid at 298 K is 12.7 mmHg

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A substance has the following properties: AHfus 10.0 kJ/mol AHvap=20.0 kJ/mol Cp (solid) = 60. J mol-¹ K-¹ Cp (liquid) = 30. J mol-¹ K-¹ Cp (gas) = 60. J mol-¹ K-¹ =

Consider the following data for an unknown substance X: AHvap 19.00 kJ/mol Specific heat capacity of liquid = 2.10 J/g °C Boiling point = 66.0°C Molar mass = 119.0 g/mol When the temperature of 1.000 mole of X(g) is lowered from 91.0°C to form X(1) at 41.0°C, 30.38 kJ of heat is released. Calculate the specific heat сараcity of X(g). Specific heat capacity = J/g °C Submit Answer Try Another Version 10 item attempts remaining 11 33°F 12 Tch

9 Consider the following phase change equilibrium: CHCI3 (s)=CHCIl3 (1) If AH° is 9.73 kJ/mol and AS° is 43.39 J/mol K, determine the melting point of CHCI3 in K? Do not report units in your answer. Report you answer as a whole number (no places past the decimal point) Type your answer...

Consider the data in the table. Compound Melting point (°C) AHrus (kJ/mol) Boiling point (°C) AH,ap (kJ/mol) HF -83.11 4.577 19.54 25.18 HCI -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 ASs and AS for HF. vap ASs = J/(K - mol) ASvap J/(K - mol) Determine the entropy change when 8.40 mol HF(s) melts at atmospheric pressure. AS = J/K