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13. Liquids, Solids & Intermolecular Forces

Heating and Cooling Curves

13. Liquids, Solids & Intermolecular Forces

Heating and Cooling Curves

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Heating and Cooling Curves Concept 1

Heating and Cooling Curves Concept 1

Heating and Cooling Curves Concept 2

Heating and Cooling Curves Concept 2

Heating and Cooling Curves Example 1

Heating and Cooling Curves Example 1

Heating and Cooling Curves Concept 3

Heating and Cooling Curves Concept 3

Heating and Cooling Curves Example 2

Heating and Cooling Curves Example 2

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Heating Curves Temperature Energy Graphs | GCSE Physics

Heating Curves Temperature Energy Graphs | GCSE Physics

The Heating and Cooling Curves.

The Heating and Cooling Curves.

Heating Curves Tutorial: How to Calculate enthalpy changes in Heating & Cooling | Crash Chemistry

Heating Curves Tutorial: How to Calculate enthalpy changes in Heating & Cooling | Crash Chemistry

Crash Chemistry Academy

Phase Changes, Heats of Fusion and Vaporization, and Phase Diagrams

Phase Changes, Heats of Fusion and Vaporization, and Phase Diagrams

Professor Dave Explains

Heating Curve and Cooling Curve of Water - Enthalpy of Fusion & Vaporization

Heating Curve and Cooling Curve of Water - Enthalpy of Fusion & Vaporization

The Organic Chemistry Tutor

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Practice this topic

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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Multiple Choice

If 53.2kJ of heat are added to a 15.5g ice cube at - 5.00 ^oC, what will be the resulting state and temperature of the substance?

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Multiple Choice

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.

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.

Textbook Question

If 42.0 kJ of heat is added to a 32.0-g sample of liquid meth-ane under 1 atm of pressure at a temperature of -170°C, what are the final state and temperature of the methane once the system equilibrates? Assume no heat is lost to the surroundings. The normal boiling point of methane is -161.5 °C. The specific heats of liquid and gaseous methane are 3.48 and 2.22 J/g-K, respectively. [Section 11.3]

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Textbook Question

Consider a compound that has a melting point at 65 °C and a boiling point at 175 °C. Which of the following images represents a heating curve for the compound from 40 °C to 200 °C? (LO 11.5)

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Textbook Question

Why is the heat of sublimation, ΔHsubl, equal to the sum of ΔHvap and ΔHfusion at the same temperature?

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Textbook Question

Name the phase transition in each of the following situa- tions and indicate whether it is exothermic or endother- mic: (d) Molten lava from a volcano turns into solid rock.

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Textbook Question

Name the phase transition in each of the following situa- tions and indicate whether it is exothermic or endother- mic: (c) Rubbing alcohol in an open container slowly disappears.

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Textbook Question

Ethyl chloride (C2H5Cl) boils at 12 °C. When liquid C2H5Cl under pressure is sprayed on a room-temperature (25 °C) surface in air, the surface is cooled considerably. (b) Assume that the heat lost by the surface is gained by ethyl chloride. What enthalpies must you consider if you were to calculate the final temperature of the surface?

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Textbook Question

For many years drinking water has been cooled in hot cli- mates by evaporating it from the surfaces of canvas bags or porous clay pots. How many grams of water can be cooled from 35 to 20 °C by the evaporation of 60 g of water? (The heat of vaporization of water in this temperature range is 2.4 kJ/g. The specific heat of water is 4.18 J/g-K).

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Textbook Question

Mercury has mp = -38.8 °C and bp = 356.6 °C. What,if any, phase changes take place under the following condi-tions at 1.0 atm pressure? (a) The temperature of a sample is raised from -30 °C to 365 °C.

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Textbook Question

How much energy in kilojoules is needed to heat 5.00 g of ice from -11.0 °C to °30.0 °C? The heat of fusion of water is 6.01 kJ>mol, and the m# olar heat capacity is 36.01 kJ>mol for ice and 75.4 J/K mol2 for liquid water

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Textbook Question

How much energy in kilojoules is released when 25.0 g of ethanol vapor at 93.0 °C is cooled to -11.0 °C? Ethanol has mp = -114.1 °C, bp = 78.3 °C, ΔHvap = 38.56 kJ>mol, and ΔHfusio#n = 4.93 kJ>mol. The molar heat#capacity is 112.3 J>1K mol2 for the liquid and 65.6 J>1K vapor.

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Textbook Question

Suppose that 0.95 g of water condenses on a 75.0-g block of iron that is initially at 22 °C. If the heat released during condensation goes only to warming the iron block, what is the final temperature (in °C) of the iron block? (Assume a constant enthalpy of vaporization for water of 44.0 kJ/mol.)

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Textbook Question

Suppose that 1.15 g of rubbing alcohol (C3H8O) evaporates from a 65.0-g aluminum block. If the aluminum block is initially at 25 °C, what is the final temperature of the block after the evaporation of the alcohol? Assume that the heat required for the vaporization of the alcohol comes only from the aluminum block and that the alcohol vaporizes at 25 °C.

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Textbook Question

How much energy is released when 65.8 g of water freezes?

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Textbook Question

Calculate the amount of heat required to completely sublime 50.0 g of solid dry ice (CO2) at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 kJ/mol.

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Textbook Question

An 8.5-g ice cube is placed into 255 g of water. Calculate the temperature change in the water upon the complete melting of the ice. Assume that all of the energy required to melt the ice comes from the water.

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Textbook Question

How much ice (in grams) would have to melt to lower the temperature of 352 mL of water from 25 °C to 5 °C? (Assume the density of water is 1.0 g/mL.)

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Textbook Question

The compound cholesteryl benzoate is a rod-like molecule that undergoes a phase change from the solid to the liq- uid crystal phase at 145.5 °C. When cholesteryl benzoate is mixed with cholesteryl oleyl carbonate, a molecule with a curved shape, the temperature of the solid to liquid crys- tal transition changes. Predict if the transition temperature increases or decreases and explain your reasoning.

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Textbook Question

Use the normal boiling points propane (C3H8) -42.1 °C butane (C4H10) -0.5 °C pentane (C5H12) 36.1 °C hexane (C6H14) 68.7 °C heptane (C7H16) 98.4 °C to estimate the normal boiling point of octane (C8H18). Explain the trend in the boiling points.

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Textbook Question

A sample of steam with a mass of 0.552 g and at a temperature of 100 °C condenses into an insulated container holding 4.25 g of water at 5.0 °C. Assuming that no heat is lost to the surroundings, what is the final temperature of the mixture?

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Textbook Question

Using information in Appendices B and C, calculate the minimum grams of propane, C3H8(g), that must be combusted to provide the energy necessary to convert 5.50 kg of ice at -20 °C to liquid water at 75 °C

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Textbook Question

Has the Earth's surface experienced warming as a result of increasing levels of greenhouse gases? If so, by how much?

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How much energy is released when 42.5 g of water freezes?

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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; ∆H_vap = 39.3 kJ/mol)

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Which is the process by which a gas changes to a solid: deposition, evaporation, freezing, or sublimation?

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What are greenhouse gases? How does carbon dioxide enter the atmosphere? (Site 1)

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If the heating curve is reversed, what would best describe the boiling point?

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