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. Ignition wires heat sample Water Stirrer Thermometer Insulated Sample Burning Steel outside dish sample bomb chamber Combustion (bomb) calorimeter. In an experiment, a 0.4370 g sample of benzoic acid (CH6O₂) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.043 x 10³ g of water. During the combustion the temperature increases from 22.78 to 25.08 °C. The heat capacity of water is 4.184 J-g¹ C¹. The heat capacity of the calorimeter was determined in a previous experiment to be 893.1 J. "C Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of benzoic acid based on these data. CHO₂(8)+(15/2)O₂(g) → 3H₂O(l) +7C0₂ (9) + Energy Molar Heat of Combustion= kJ/mol

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. Ignition wires heat sample Water Stirrer Thermometer Insulated Sample Burning Steel outside dish sample bomb chamber Combustion (bomb) calorimeter. In an experiment, a 0.4370 g sample of benzoic acid (CH6O₂) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.043 x 10³ g of water. During the combustion the temperature increases from 22.78 to 25.08 °C. The heat capacity of water is 4.184 J-g¹ C¹. The heat capacity of the calorimeter was determined in a previous experiment to be 893.1 J. "C Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of benzoic acid based on these data. CHO₂(8)+(15/2)O₂(g) → 3H₂O(l) +7C0₂ (9) + Energy Molar Heat of Combustion= kJ/mol

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

Could someone please help! No plagiarism Please! 3. Draw an or find an image of an endothermic reaction or an exothermic reaction. Explain what makes it the type of reaction you chose to illustrate. Include arrows to show what direction the overall enthalpy of reaction (energy of reaction) flows. 4. Ammonium nitrate dissolves in water via the following reaction: NH4NO3(s) → NH4+(aq) + NO3-(aq) The bond energies of the compounds in the reaction are as follows: NH4NO3 = 3040 kJ/mol NH4+ = 1564 kJ/mol NO3- = 1009 kJ/mol How much total energy does the reaction have, and how will the environment change when the reaction occurs? Please show all of your work
Use the following information to answer Questions 6-9: A sample of NH4NO3 with a mass of 5.0 g is dissolved in 40.1 g of deoinized water in a calorimeter. The initial temperature of the water is 21.2 oC. The final temperature of the solution is 15.4 oC. The calorimeter constant = 25.2 J/oC. Is the following statement true or false? This process is exothermic. True False
A 3.59°C increase in temperature occurs when a 0.232 g sample of benzoic acid (C7H6O2) is combusted in a bomb calorimeter. A 1.81 °C increase in temperature occurs when a 0.303 g sample of citric acid (C6H8O7) is combusted in the same bomb calorimeter. The heat of combustion of benzoic acid is -26.37 kJ/g. What is the molar heat of combustion of citric acid? Reminder: Any heats of combustion will be negative since these are exothermic reactions.
The flame in a torch used to cut metal is produced by burning acetylene (C2H2)(26.04 g/mol) in pure oxygen. Assuming the combustion of 1 mole of acetylene releases 1251 kJ of heat, what mass of acetylene is needed to cut through a piece of steel if the process requires 22.5 × 104 kJ of heat? 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(g) ΔH = –2502 kJ
When 3.8 g A are reacted with 8.5 g D, according to the balanced chemical equation below, 33 kJ of energy are released. Please calculate the enthalpy for this reaction when 3 moles of G are produced. 2A + 3D = 2Z + 3G given molar masses: A = 141.8 g/mole D = 63.996 g/ mole Z = 4.032 g/ mole G = 56.028 g/ mole
A chemist burned a sample of coal in a bomb calorimeter. Her results are below. Calorimeter's Heat Capacity 7.264 kJ/°C Mass of Coal Initial Temperature Final Temperature 0.100 g 22.07°C 25.37°C The sample of coal that the chemist placed in the bomb was dry but when she finished the test there was a small amount of water in the bomb. Where did this water come from and how does it affect her result? The water came from the water surrounding the bomb so her measured heat of combustion is for a closed system. The water was a product of combustion so her measured heat of combustion is for an open system. The water came from the water surrounding the bomb so her measured heat of combustion is for an open system. The water was a product of combustion so her measured heat of combustion is for a closed system.
True or False: The test tube in which a chemical reaction is taking place feels warmer to the touch. The reaction is endothermic.