unknown liquid (MM = 83.21 g/mol) at 19.2 °C to a gas at s (g) 0.932 J/(g-°C) 93.5 °C? T. 57.3 °C AH 22.5 kH/mol

How much heat (in kJ) is absorbed in the process of making 0.729 mol of CF₄ from the following reaction? C (s) + 2 F₂ (g) → CF₄ (g) ∆H° = 141.3 kJ/mol

A 459.3 gram sample of an unknown substance (MM = 92.41 g/mol) is heated from -23.1 °C to 51.8 °C. (heat capacity of solid = 2.96 J/g･°C; heat capacity of liquid = 1.75 J/g･°C; ∆Hfus = 8.04 kJ/mol; normal freezing point, Tf = 17.6 °C) How much energy (in kJ) is absorbed/released to heat the solid?

What is the change in heat (in kJ to one decimal place) when 1.75 L of H2O condenses under 1 atm pressure at 100 °C?  ΔHvap = 40.7 kJ mol–1 d(H2O) = 0.958 g mL–1 (at 100 °C)

5. When 10 g of diethyl ether is converted to vapor at its boiling point, how much heat is absorbed? (C4H100, AHvar = 15.7 kJ/mol, boiling point: 34.6°C) а. 20 КJ b. 0.2 KJ с. 2 КJ d. 200 KJ

What quantity of heat (in kJ) is absorbed in the process of making 0.889 mol of CF₄ from the following reaction? C (s) + 2 F₂ (g) → CF₄ (g) ∆H° = 141.3 kJ/mol

What is the boiling point of methanol, CH3OH: CH3OH()→ CH3OH(g) AGO = AHO- TASO AH°= 38.0 kJ mol and ASO = 113.0 J-K1-mol1 Item equation/constant O 3.0 °C O 63 °C O 75 °C O 336 °C

How hot does a thanksgiving dinner roll need to be to warm up and melt a 4.0 g 'pat' of butter? (Roll: 25 g, Csteam= 1.996 J/g°C; Tr = 32°C; Butter: Ti = 2.0°C, Tr = 32°C, Cbutter = 2.72 J/g°C, Hfusion = 32 J/g). [Remember, heat lost by roll equals heat gained by butter. Assume the specific heat of the roll is the same as the %3D specific heat of steam.]

From 25.0°C to 94.5°C, 75.1 grams of ethanol are heated. What was the energy requirement in joules?H(vap) 38.6 kJ/mol and H(fus) 4.60 kJ/mol are the heats of vaporization and fusion, respectively, for ethanol. cp (liquid) ethanol 2.46 J/g°C, cp (gas) ethanol 1.43 J/g°C, and cp (solid) ethanol 2.42 J/g°C are the specific temperatures for the three phases of ethanol. Ethanol has a molecular weight of 46. The melting point of ethanol is -114.1 °C and the boiling point is 78.4 °C.

Calculate the amount of heat (in kJ) required to raise the temperature of a 86.0 g sample of ethanol from 198.0 K to 300.0 K. The specific heat capacity of ethanol is 2.42 J/g°C. 60.0 kJ 21.2 kJ 11.9 kJ 75.6 kJ 28.4 kJ