The enthalpy of combustion of benzoic acid (CH;COOH) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be -3226.7 kJ/mol When 3.1325 g of benzoic acid are burned in a calorimeter, the temperature rises from 20.84°C to 26.67°C. What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly 2250 g.) KJPC

The enthalpy of combustion of benzoic acid (CH;COOH) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be -3226.7 kJ/mol When 3.1325 g of benzoic acid are burned in a calorimeter, the temperature rises from 20.84°C to 26.67°C. What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly 2250 g.) KJPC

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...

See similar textbooks

Similar questions

When methanol, CH, OH, is burned in the presence of oxygen gas, O,, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH, OH(g) + 0,(g) → CO,(g) + 2 H,O(1) ΔΗ --764 kJ How much methanol, in grams, must be burned to produce 837 kJ of heat?
Sucrose is common sugar. It is produced naturally in plants, from which table sugar is refined. A sample of sucrose (C12H22O11) with a mass of 2.68 g is burned in a bomb calorimeter. The heat capacity of this calorimeter is 8.91 kJ/°C. The temperature changes from 23.0°C to 30.5°C. Calculate the heat of combustion of sucrose in kilojoules per mole. Question options: a. -8.54 x 103 b. 4.64 x 105 c. 2.01x 10-4 d. -1.88 x 102
The heat capacity of a bomb calorimeter was determined by burning 6.85 g of methane (energy of combustion = -803 kJ/mol CH4) in the bomb. The temperature changed by 11.1°C. (a) What is the heat capacity of the bomb? kJ/°C (b) A 14.7-g sample of ethanol (C₂H5OH) produced a temperature increase of 12.8°C in the same calorimeter. What is the energy of combustion of ethanol (in kJ/mol)? kJ/mol
When 1.836 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?
A student has a coffee-cup calorimeter with 50.0 g of water at 21.5oC. They introduce 15.525 g of magnesium metal initially at 100.0oC. The final temperature of the calorimeter came to 27.2oC. What is the value of T magnesium in kelvin?
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 6.10 g of urea,(NH2)2CO (g), burns to produce CO2 (g), N2 (g) and H2O (l) 67.8 kJ of heat energy are released in a bomb calorimeter. What is the energy released in the burning of one mole of urea? Using this, what is the enthalpy of formation of urea?
The enthalpy change for the oxidation of butane, C4H₁0, is measured by calorimetry. C4H10 (g) + 13/2 O2(g) → 4 CO2 (g) +5 H₂O(l) A₂H = -2877.6 kJ/mol-rxn Use this value, along with the standard enthalpies of formation of CO2(g) and H₂O(l) (-393.509 kJ/mol and -285.83 kJ/mol respectively), to calculate the enthalpy of formation of butane, C4H10, in kJ/mol. Enthalpy of formation = Submit Answer OCT 30 Try Another Version tv kJ/mol S4 I all 9 item attempts remaining Cengage Learning | Cengage Technical Support A MacBook Pro 7 ( O 04
The combustion of toluene has a AErxn of -3.91 x 10³ kJ/mol. When 1.30 g of toluene (C7H8) undergoes combustion in a bomb calorimeter, the temperature rises from 22.80 °C to 36.11 °C. Find the heat capacity of the bomb calorimeter. Express your answer using three significant figures. Ccal = 17| ΑΣΦ ? kJ/°C
The enthalpy of combustion of benzoic acid is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be -3226.7 kJ/mol. When 1.9862 g of benzoic acid are burned in a calorimeter, the temperature rises from 21.84 degrees Celsius to 25.67 degrees Celsius. What is the heat capacity of the bomb in kJ/degrees Celsius?
A student is attempting to determine the heat capacity of a Styrofoam cup calorimeter by pouring hot water into a Styrofoam cup containing cold water. The student determined the mass of the cold water to be 21.2455 g and its initial temperature to be 20.36 °C. The mass of the hot water was 24.2646 g and its initial temperature as 34.54 °C. The final temperature of the water after mixing was determined to be 24.57°C. The specific heat capacity of the water is 4.184 J/(g•°C). What is the heat capacity of the Styrofoam cup calorimeter? Assume the temperature of the calorimeter is the same temperature as the cold water. 4.184 J/°C 132.5 J/°C