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8. Thermochemistry

Constant-Pressure Calorimetry

8. Thermochemistry

Constant-Pressure Calorimetry

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Constant-Pressure Calorimetry

Constant-Pressure Calorimetry

Constant-Pressure Calorimetry Example 1

Constant-Pressure Calorimetry Example 1

Constant-Pressure Calorimetry

Constant-Pressure Calorimetry

Constant-Pressure Calorimetry Example 2

Constant-Pressure Calorimetry Example 2

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Chemistry - Thermochemistry (31 of 37) Constant Pressure Calorimeter: Ex. 2

Chemistry - Thermochemistry (31 of 37) Constant Pressure Calorimeter: Ex. 2

Michel van Biezen

Coffee Cup Calorimetry Examples (Constant Pressure)

Coffee Cup Calorimetry Examples (Constant Pressure)

Samantha Ramaswamy

Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry

Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry

Melissa Maribel

Chapter 09 - 16 - Constant Pressure Calorimetry (coffee cup)

Chapter 09 - 16 - Constant Pressure Calorimetry (coffee cup)

Calorimetry (Constant-Pressure Calorimeter)

Calorimetry (Constant-Pressure Calorimeter)

The Science Classroom

Chemistry - Thermochemistry (26 of 37) Constant Pressure Calorimeter

Chemistry - Thermochemistry (26 of 37) Constant Pressure Calorimeter

Michel van Biezen

CHEMISTRY 101 - Constant Pressure Calorimetry

CHEMISTRY 101 - Constant Pressure Calorimetry

Showing 7 of 7 videos

Practice this topic

Multiple Choice

A 115.6 g piece of copper metal at 182.5 ºC is placed into 120.0 mL of methylene chloride at 31.0 ºC within a coffee-cup calorimeter. If the final temperature of the solution is 50.3 ºC, what is the specific heat of methylene chloride? Assume the calorimeter absorbs a negligible amount of heat. The specific heat of copper is 4.184 J/g ∙ ºC and the density of methylene chloride is 1.33 g/cm³.

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Multiple Choice

You place 75.0 mL of 0.100 M NaOH in a calorimeter at 25.00 ºC and carefully add 55.0 mL of 0.200 M HNO₃, also at 25.00 ºC. After stirring, the final temperature is 53.35 ºC. Calculate the enthalpy ∆H_rxn (in J/mol) for the formation of water. (Specific heat capacity, Cs, and density of the solution:4.184 J/g∙K and 1.00 g/mL).

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Multiple Choice

When gasoline is burned at constant pressure, a certain amount of heat is emitted and work is done. Which of the following must be true?

Textbook Question

When an 18.6-g sample of solid potassium hydroxide dissolves in 200.0 g of water in a coffee-cup calorimeter (Figure 5.18), the temperature rises from 23.7 to 44.5 °C. (a) Calculate the quantity of heat (in kJ) released in the reaction.

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Textbook Question

When an 18.6-g sample of solid potassium hydroxide dissolves in 200.0 g of water in a coffee-cup calorimeter (Figure 5.18), the temperature rises from 23.7 to 44.5 °C. (b) Using your result from part (a), calculate H (in kJ>mol KOH) for the solution process. Assume that the specific heat of the solution is the same as that of pure water.

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Textbook Question

Instant hot packs contain a solid and a pouch of water. When the pack is squeezed, the pouch breaks and the solid dis- solves, increasing the temperature because of the exothermic reaciton. The following reaction is used to make a hot pack: H2O LiCl1s2 ¡ Li 1aq2 + Cl 1aq2 ∆H = -36.9 kJ. What is the final temperature in a squeezed hot pack that contains 25.0 g of LiCl dissolved# in 125 mL of water? Assume a specific heat of 4.18 J>1g °C2 for the solution, an initial temperature of 25.0 °C, and no heat transfer between the hot pack and the environment.

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Textbook Question

When 1.50 g of magnesium metal is allowed to react with 200 mL of 6.00 M aqueous HCl, the temperature rises from 25.0 °C to 42.9 °C. Calculate ΔH in kilojoules for the reaction, assumign that the heat capacity of the calorimeter is 776 J/°C, that the specific heat of the final soltuion is the same as that of water [4.18 J(g·°C)] and that the density of the solution is 1.00 g/mL

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Textbook Question

A 110.0 g piece of molybdenum metal is heated to 100.0 °C and placed in a calorimeter that contains 150.0 g of water at 24.6 °C. The system reaches equilibirum at a final temeprature of 28.0 °C. Calcualte the specific heat of molybdenum metal in J/g·°C. The specific heat of water is 4.18 J/g·°C

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Textbook Question

Citric acid has three dissociable hydrogens. When 5.00 mL of 0.64 M citric acid and 45.00 mL of 0.77 M NaOH are mixed at an initial temperature of 26.0 °C, the temperature rises to 27.9 °C as the citric acid is neutralized. The combined mixture ahs a mass of 51.6 g and a specific heat of 4.0 J/(g·°C). Assuming that no heat is transferred to the surroundings, cal- culate the enthalpy change for the reaction of 1.00 mol of cit- ric acid in kJ. Is the reaction exothermic or endothermic?

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Textbook Question

A coffee-cup calorimeter of the type shown in Figure 5.18 contains 150.0 g of water at 25.2 °C. A 200-g block of silver metal is heated to 100.5 °C by putting it in a beaker of boiling water. The specific heat of Ag(s) is 0.233J>1g # K2. The Ag is added to the calorimeter, and after some time the contents of the cup reach a constant temperature of 30.2 °C. (d) What would be the final temperature of the system if all the heat lost by the silver block were absorbed by the water in the calorimeter?

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Textbook Question

A coffee-cup calorimeter of the type shown in Figure 5.18 contains 150.0 g of water at 25.2 °C. A 200-g block of silver metal is heated to 100.5 °C by putting it in a beaker of boiling water. The specific heat of Ag(s) is 0.233J>1g # K2. The Ag is added to the calorimeter, and after some time the contents of the cup reach a constant temperature of 30.2 °C. (b) Determine the amount of heat gained by the water. The specific heat of water is 4.184 J>1g # K2.

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Textbook Question

A coffee-cup calorimeter of the type shown in Figure 5.18 contains 150.0 g of water at 25.2 °C. A 200-g block of silver metal is heated to 100.5 °C by putting it in a beaker of boiling water. The specific heat of Ag(s) is 0.233J>1g # K2. The Ag is added to the calorimeter, and after some time the contents of the cup reach a constant temperature of 30.2 °C. (a) Determine the amount of heat, in J, lost by the silver block.

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Textbook Question

A sample of a hydrocarbon is combusted completely in O21g2 to produce 21.83 g CO21g2, 4.47 g H2O1g2, and 311 kJ of heat. (a) What is the mass of the hydrocarbon sample that was combusted?

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Textbook Question

An empty 4.00-L steel vessel is filled with 1.00 atm of CH41g2 and 4.00 atm of O21g2 at 300 °C. A spark causes the CH4 to burn completely, according to the equation CH41g2 + 2 O21g2¡CO21g2 + 2 H2O1g2 ΔH° = -802 kJ (b) What is the final temperature inside the vessel after combustion, assuming that the steel vessel has a mass of 14.500 kg, the mixture of gases has an average molar heat capacity of 21 J>1mol # °C2, and the heat capacity of steel is 0.449 J>1g # °C2?

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Textbook Question

(c) Assume that a chunk of potassium weighing 7.55 g is dropped into 400.0 g of water at 25.0 °C. What is the final temperature of the water if all the heat released is used to warm the water?

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When a 4.25g sample of solid ammonium

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