Compound Melting point ("C) AHs (kJ/mol) Boiling point ("C) AHp (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 A.Sus and A.Svup for HF. AStus = J/(K mol) + TOOLS X10 A.Svap = J/(K mol) Determine the entropy change when 7.20 mol HF(g) condenses at atmospheric pressure. J/K AS =

How long (in seconds) would it take a 50.0 watt (1 watt = 1 J/s) heater to melt 10.02 g of Au(s) initially at its freezing point (1064 °C) to the boiling point (2807 °C) and then to completely vaporize it?

A solid will melt to its liquid phase if enough heat is applied. A udy True O Search O False

Isopropyl alcohol, also known as rubbing alcohol, can be used for a variety of cleaning and disinfecting purposes. How much energy (kJ) is needed to heat 25.0 g of isopropyl alcohol from -25.0°C to +90.0°C? Molar mass 60.1 g/mol Boiling point 82.5 °C Melting point -89.0 °C kJ Heat of vaporization, AHvap 39.85 kJ/mol Round your final answer to 2 Specific heat capacity, liquid 1.71 J/(g K) significant digits. Specific heat capacity, gas 2.49 J/(g K)

CH4(g) +20₂(g) AH₁-890 kJ -890 kJ -90 kJ -800 kJ What is the heat necessary to evaporate one mole of water at constant pressure? +90 kJ AH₂ =-800 kJ +45 kJ CO₂(g) + 2H₂O(g) CO₂(g) + 2H₂O(1) AH₂ = ?

5. Is the melting temperature of a substance different from its freezing temperature? Define the process of melting:

How much heat, in joules and in calories, must be added to a 89.1 g chromium block with a specific heat of 0.450 J/g·°C to increase its temperature from 25°C to its melting temperature of 1907°C?

Consider the data in the table. Compound Melting point (°C) AHfus (kJ/mol) Boiling point (°C) AHvap (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 ASfus and A.Svap for HBr. ASfus= 13 ASvap 93 Determine the entropy change when 6.90 mol HBr(1) freezes at atmospheric pressure. 355 AS= J/(K-mol) J/(K - mol) J/K Question Source: McQuarrie, Rock, And Gallogly 4e General Chemistry | Publisher Universit

Based on the thermodynamic properties provided for water, determine the amount of energy released for 50.00 g of water to go from 62.0 °C to -17.0 °C. Property Melting point Boiling point 12.3 AHfus Hvap Cp (s) Cp (1) Cp (g) kJ Value 0.0 100.0 6.01 40.67 37.1 75.3 33.6 Units. °C °C kJ/mol kJ/mol J/mol · °C J/mol · °C J/mol °C

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 ASfas and ASap for HF. ASfus = J/(K · mol) ASvap J/(K - mol) Determine the entropy change when 9.50 mol HF(g) condenses at atmospheric pressure. AS = J/K