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13. Liquids, Solids & Intermolecular Forces

Heating and Cooling Curves

General Chemistry

13. Liquids, Solids & Intermolecular Forces

Heating and Cooling Curves

4:11 minutes

Open Question

What quantity of heat, in kj, is required to convert 50.0 g of ethanol (C₂H₅OH) at 23.0°C to a vapor at 78.3°C (its boiling point)? (specific heat capacity of ethanol = 2.46 J/g • c; ∆H_vap = 39.3 kJ/mol)

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Multiple Choice

How much energy (kJ) is required to convert a 76.4 g acetone (MM = 58.08 g/mol) as a liquid at -30°C to a solid at -115.0°C?

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Calculate the volume (mL) of acetone, C₃ H₆ O, (density = 0.786 g/mL) that can be vaporized at its normal boiling point with 345 kJ of heat. ΔH_vap for acetone is 29.1 kJ/mol.

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Multiple Choice

Determine the vapor pressure (atm) of rubbing alcohol (isopropanol) at 20.0℃. The normal boiling point of isopropanol is 82.3℃ and the heat of vaporization (ΔH_vap) is 39.9 kJ/mol.

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Open Question

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Open Question

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Open Question

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Open Question

The human body obtains 915 kJ of energy from a candy bar. If this energy were used to vaporize water at 100.0 °C, how much water (in liters) could be vaporized? (Assume the density of water is 1.00 g/mL.)

Open Question

A 100.0-mL sample of water is heated to its boiling point. How much heat (in kJ) is required to vaporize it? (Assume a density of 1.00 g/mL.)

Open Question

How much heat (in kJ) is required to warm 10.0 g of ice, initially at -10.0 °C, to steam at 110.0 °C? The heat capacity of ice is 2.09 J/g°C, and that of steam is 2.01 J/g°C.

Open Question

How much heat (in kJ) is evolved in converting 1.00 mol of steam at 145 °C to ice at -50 °C? The heat capacity of steam is 2.01 J/g°C, and that of ice is 2.09 J/g°C.

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Four ice cubes at exactly 0 °C with a total mass of 53.5 g are combined with 115 g of water at 75 °C in an insulated container. If no heat is lost to the surroundings, what is the final temperature of the mixture?

Open Question

Draw a heating curve (such as the one in Figure 11.36) for 1 mole of methanol beginning at 170 K and ending at 350 K. Assume that the values given here are constant over the relevant temperature ranges. Melting point: 176 K, Boiling point: 338 K, ΔH_fus: 2.2 kJ/mol, ΔH_vap: 35.2 kJ/mol, C_s,solid: 105 J/mol·K, C_s,liquid: 81.3 J/mol·K, C_s,gas: 48 J/mol·K.

Open Question

Draw a heating curve (such as the one in Figure 11.36) for 1 mol of benzene beginning at 0 °C and ending at 100 °C. Assume that the values given here are constant over the relevant temperature ranges: Melting point 5.4 °C, Boiling point 80.1 °C, ΔHfus 9.9 kJ/mol, ΔHvap 30.7 kJ/mol, Cs,solid 118 J/mol⋅K, Cs,liquid 135 J/mol⋅K, Cs,gas 104 J/mol⋅K.

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What quantity of heat, in kj, is required to convert 50.0 g of ethanol (C₂H₅OH) at 23.0°C to a vapor at 78.3°C (its boiling point)? (specific heat capacity of ethanol = 2.46 J/g • c; ∆Hvap = 39.3 kJ/mol)

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Heating and Cooling Curves practice set

What quantity of heat, in kj, is required to convert 50.0 g of ethanol (C₂H₅OH) at 23.0°C to a vapor at 78.3°C (its boiling point)? (specific heat capacity of ethanol = 2.46 J/g • c; ∆H_vap = 39.3 kJ/mol)