A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of 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 0.981-g sample of L-ascorbic acid (CgHgO6) in a bomb calorimeter containing 1060. g of water. The temperature increases from 24.80 °C to 27.30 °C. The heat capacity of water is 4.184 Jgl-c•!. The molar heat of combustion is -2340. kJ per mole of L-ascorbic acid. C,H2O6(s) + 5 O,(g) -6 CO,(g) + 4 H,O(1) + Energy Calculate the heat capacity of the calorimeter. heat capacity of calorimeter - | J/°C

A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of 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 0.981-g sample of L-ascorbic acid (CgHgO6) in a bomb calorimeter containing 1060. g of water. The temperature increases from 24.80 °C to 27.30 °C. The heat capacity of water is 4.184 Jgl-c•!. The molar heat of combustion is -2340. kJ per mole of L-ascorbic acid. C,H2O6(s) + 5 O,(g) -6 CO,(g) + 4 H,O(1) + Energy Calculate the heat capacity of the calorimeter. heat capacity of calorimeter - | J/°C

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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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.
A chemist wastes a delicious brownie by burning it in a bomb calorimeter. Before burning, the brownie weighed 18.19 grams. During the combustion process in the bomb calorimeter, the heat of the calorimeter increased by 8.75 ∘C. The known heat capacity of the calorimeter that was used was 33.53 kJ/∘C. What is the energy content, in kJ/g, of this brownie? Enter your answer with no units.
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter.In the laboratory a general chemistry student finds that when 9.01 g of K2SO4(s) are dissolved in 112.40 g of water, the temperature of the solution drops from 23.35 to 20.44 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.88 J/°C.Based on the student's observation, calculate the enthalpy of dissolution of K2SO4(s) in kJ/mol.Assume the specific heat of the solution is equal to the specific heat of water.
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The standard state of carbon is graphite. ΔH°f,diamond is +1.896 kJ/mol. Diamonds are normally weighed in units of carats, where 1 carat = 0.200 g Determine the standard enthalpy of the reaction for the conversion of a 3.61 -carat diamond into an equivalent mass of graphite.
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