2. In studying the energy generated by a person, you may view the person roughly as a constant pressurcalorimeter using sugar (i.e., sucrose, C₁2H₂2O11) to generate power. The reaction of table sugar incalorimeter is given by+Ch. 9 Sl....pdfC12H22O11(s)+120₂(g) →12CO₂(g)+11H₂O+heat.C.a. What is the heat released by consuming one mole of sugar (C₁2H22O11) in thisb. Calculate the enthalpy of combustion persugar utilization.moleDoes the result of your calculation makeIwi(540Karak1411 Mde20091APfikTour of1way?20

Answered: Image /qna-images/answer/ca68422e-1e27-4194-bef1-68888e1b2f95.jpg

2. In studying the energy generated by a person, you may view the person roughly as a constant pressur calorimeter using sugar (i.e., sucrose, C12H22O11) to generate power. The reaction of table sugar in calorimeter is given by Ha Ishrut dan + ay siy C. C₁2H22O11(s)+120₂(g) →12CO₂(g)+11H₂O+heat. 22-Byroon m a. What is the heat released by consuming one mole of sugar (C12H22O11) in this way? b. gratis 9 Calculate the enthalpy of combustion per mole of sugar utilization. Does the result of your calculation make sense? HOUS #garran banyung 10 Pachet

2. In studying the energy generated by a person, you may view the person roughly as a constant pressur calorimeter using sugar (i.e., sucrose, C12H22O11) to generate power. The reaction of table sugar in calorimeter is given by Ha Ishrut dan + ay siy C. C₁2H22O11(s)+120₂(g) →12CO₂(g)+11H₂O+heat. 22-Byroon m a. What is the heat released by consuming one mole of sugar (C12H22O11) in this way? b. gratis 9 Calculate the enthalpy of combustion per mole of sugar utilization. Does the result of your calculation make sense? HOUS #garran banyung 10 Pachet

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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At constant volume, the heat of combustion of a particular compound, compound A, is −3520.0 kJ/mol.−3520.0 kJ/mol. When 1.439 g1.439 g of compound A (molar mass =112.71 g/mol)=112.71 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.391 ∘C.6.391 ∘C. What is the heat capacity (calorimeter constant) of the calorimeter?
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A chemist carefully measures the amount of heat needed to raise the temperature of a 0.38 kg sample of C,HgO, from 53.1 °C to 64.4 °C. The experiment shows that 6.73 × 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
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Having just invented a new type of calorimeter, Dr. Covey needs to determine the heat capacity of the calorimeter. She carries out the following experiment to do this: Her empty calorimeter is at a temperature of 25.0ºC. She adds 58.606 grams of water at a temperature of 86.4ºC to the empty calorimeter and the final temperature of the calorimeter and the water is 41.9ºC. Based on this experiment, what is the heat capacity of her calorimeter assuming units of J/ºC? Enter your answer with at least 3 sig figs.
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy available from foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.983-g sample of glutaric acid (C;HgO4) in a bomb calorimeter containing 1170. g water. The temperature increases from 24.10 °C to 26.90 °C. The specific heat capacity of water is 4.184 J g-1 °C-!. The combustion enthalpy is -2151 kJ/mol glutaric acid. C5H3O4(s) + 5 02(g) 5 CO2(g) + 4 H2O(1) A,H° = -2151 kJ/mol Calculate the heat capacity of the calorimeter. heat capacity of calorimeter = J/°C
Having just invented a new type of calorimeter, Dr. Cox needs to determine the heat capacity of the calorimeter. She carries out the following experiment to do this: Her empty calorimeter is at a temperature of 25.0ºC. She adds 32.502 grams of water at a temperature of 72.5ºC to the empty calorimeter and the final temperature of the calorimeter and the water is 39.5ºC. Based on this experiment, what is the heat capacity of her calorimeter assuming units of J/ºC? Enter your answer with at least 3 sig figs.
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