In an experiment, a 0.7520 g sample of 1,2-benzenediol (C6H6O₂) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.284 x 10³ g of water. During the combustion the temperature increases from 27.68 to 30.74 °C. The heat capacity of water is 4.184 J·g-¹. °C-¹. The heat capacity of the calorimeter was determined in a previous experiment to be 818.2 J. C-¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 1,2-benzenediol based on these data. C6H6O₂ (s) + (13/2)O₂(g) → 3H₂O(l) + 6CO2 (g) + Energy kJ/mol Molar Heat of Combustion = Previous Next

In an experiment, a 0.7520 g sample of 1,2-benzenediol (C6H6O₂) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.284 x 10³ g of water. During the combustion the temperature increases from 27.68 to 30.74 °C. The heat capacity of water is 4.184 J·g-¹. °C-¹. The heat capacity of the calorimeter was determined in a previous experiment to be 818.2 J. C-¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 1,2-benzenediol based on these data. C6H6O₂ (s) + (13/2)O₂(g) → 3H₂O(l) + 6CO2 (g) + Energy kJ/mol Molar Heat of Combustion = Previous Next

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A 1.200 g sample of ZnCO3 (s) dissolved in 40.0 mL of a dilute HCl solution (density = 1.10 g/mL) in a coffee cup calorimeter, producing CO2 (g), liquid water and ZnCl2 (aq). The temperature of the solution changes from 24.32 oC to 25.49 oC. The resulting solution has a specific heat of 4.18 J/goC. What would be a balanced equation for this reaction.
(b) In one experiment, a 25 g sample of an alloy was heated to a certain temperature. The heated alloy was then dropped into a beaker containing 90 g of water at 25.32 °C. The temperature of the water rose to a final value of 27.18 °C. Predict the final temperature that the alloy is being heated at the beginning of the experiment. Given that the heat capacity of water and alloy are 4.184 JgC and 0.3847 Jg l°C-' respectively.
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 1.4710 g sample of maleic acid (C4H4O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1159 g of water. During the combustion the temperature increases from 22.46 to 25.59 °C. The heat capacity of the calorimeter, not including the surrounding water, was determined in a previous experiment to be 852.2 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of maleic acid based on these data. Assuming that no energy is lost to the surroundings, what is the molar heat of combustion of maleic acid, based on these data? (in kJ/mol). C4H4O4(s) + 3O2(g) → 2 H2O(l) + 4 CO2(g) + Energy
A 1.75 g sample of zinc metal is reacted with 128 g of 1.10 M hydrochloric acid solution in a constant-pressure calorimeter. The resulting solution changes in temperature from 22.58 °C to 22.97 °C. The hydrochloric acid is in excess. Based on this information, and estimating the solution's heat capacity as 4.18 Jg1 °C, what is the amount of heat, in joules, transferred in this reaction?
A chemist wastes a delicious brownie by burning it in a bomb calorimeter. Before burning, the brownie weighed 21.80 grams. During the combustion process in the bomb calorimeter, the heat of the calorimeter increased by 7.87 ∘C. The known heat capacity of the calorimeter that was used was 42.73 kJ/∘C. What is the energy content, in kJ/g, of this brownie? (Enter your answer with no units. Since we are describing the energy content of the brownie, please ENTER THIS NUMBER AS A POSITIVE NUMBER, not a negative number!)
the molar heat capacity of iron is 25.10 J mol –1 K–1 . A 25.0 g ball is heated until it is glowing red (to a temperature of 400.°C). It is dropped into a 50.0 mL container of water at 25.0°C. If the density of water is 0.997 g mL–1 , and the molar heat capacity of water is 4.186 J g–1 K–1 , what temperature (in K) will the ball and water equilibrate to? A) 338 B) 300 C) 317 D) 359 E) 342
The combustion of 1.00mol of glucose (C6H12O6) liberates 2820 kJ of heat. If 1.64g of glucose is burned in a calorimeter containing 788 g of water, and the temperature of the assembly increases from 20.10oC to 24.16oC, what is the heat capacity of the calorimeter in kJ/oC? MW of glucose is 180 g/mol.
A chemist carefully measures the amount of heat needed to raise the temperature of a 0.88 kg sample of C,H0, from 35.8 °C to 51.4 °C. The experiment shows that 2.34 × 10* J of heat are needed. What can the chemist report for the molar heat capacity of C,H00,? Round your answer to 2 significant digits. |J-mol 1 - 1 •K х10
When 1.366 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?
In an experiment, a 0.5002 g sample of tridecanedioic acid ( C13 H24 O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.165 × 10³ g of water. During the combustion the temperature increases from 21.99 to 24.52 °C. The heat capacity of water is 4.184 J·g¯¹. °C-¹. The heat capacity of the calorimeter was determined in a previous experiment to be 904.0 J. °C¯¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of tridecanedioic acid based on these data. C13H24 O4(s) + 17O2 (g) → 12H₂O(l) + 13CO2 (g) + Energy kJ/mol Molar Heat of Combustion =
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A chemist carefully measures the amount of heat needed to raise the temperature of a 0.34 kg sample of C,H¸0 from -1.5 °C to 18.1 °C. The experiment shows that 1.09 × 10* J of heat are needed. What can the chemist report for the molar heat capacity of C,H,O? Round your answer to 2 significant digits. J• mol -1 1 ·K x10