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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A) When 1.911 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.410 °C to 26.630 °C. If the heat capacity of the calorimeter is 4.900 kJ/ °C, what is the heat of combustion of sucrose, in kJ/mol? And B) A 90.0 g piece of metal, initially at 98.60 °C, is placed into 120.0 g of water initially at 24.30 °C. If the final temperature of the water is 34.00 °C, what is the specific heat of the metal? (The specific heat of water is 4.184 J/g･ °C).
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 0.90 g of CaCl2(s) are dissolved in 102.10 g of water, the temperature of the solution increases from 22.90 to 24.48 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.79 J/°C.Based on the student's observation, calculate the enthalpy of dissolution of CaCl2(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water.ΔHdissolution = kJ/mol
A 1.261 g sample of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and its contents increase from 25.39 °C to 28.44 °C. The heat capacity (calorimeter constant) of the calorimeter is 27.69 kJ/ °C, what is the heat of combustion per gram of the material? heat of combustion: kJ/g
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 5.26 g of CsClO4(s) are dissolved in 103.30 g of water, the temperature of the solution drops from 22.98 to 19.81 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.79 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of CsClO4(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water.
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?
The complete combustion of salicylic acid releases 21.90 kJ of energy per gram of salicylic acid.In a particular bomb calorimeter (initially at room temperature), the combustion of 0.2745 g of salicylic acid, in the presence of excess oxygen, causes the temperature of the calorimeter to rise by 1.85 °C.When a 0.2999-g sample of an unknown organic substance is similarly burned in the same calorimeter, the temperature rises by 3.59 °C.What is the energy of combustion per unit mass of the unknown substance?
10 A student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 37.48°C. The specific heat capacity of water is 4.184 J and the density of water is g. °C 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = °C
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!)
1. Magnesium solid reacts with aqueous hydrochloric acid to form the Mg2+ ion in solution. In an experiment, 60.0 mL of aqueous HCl was mixed with 0.1297 g of magnesium solid in a double Styrofoam cup calorimeter. The reaction caused the temperature of the substances in the calorimeter to rise 10.02°C. Assume the density and specific heat of the HCl solution is that of water, 1.00 g/mL and 4.184 J/g °C, respectively. The specific heat of magnesium is 1.02 J/g °C. a. Write the balanced chemical equation for this reaction. b. Calculate the heat of this reaction, AHrxn, in kJ. c. Calculate the heat of this reaction per mole of Mg2+ formed, AHxn/mole Mg²+. d. The literature value of this reaction is -466.85 kJ/mole. Calculate the percent deviation of the experimental value from the literature value.
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 0.79 g of KOH(s) are dissolved in 104.10 g of water, the temperature of the solution increases from 24.69 to 26.63 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.58 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of KOH(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. kJ/mol AH dissolution = BrookaCom Cengage Leaming Thermometer Cardboard or Styrofoam lid Nested Styrofoam cups Reaction occurs in solution.
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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 0.461-g sample of 2-naphthylacetic acid (C12H1002) in a bomb calorimeter containing 1150. g water. The temperature increases from 24.70 °C to 27.20 °C. The specific heat capacity of water is 4.184 J g1 oC-1. The combustion enthalpy is -5779 kJ/mol 2-naphthylacetic acid. C12H1002(s) + 27/2 02(g) –→12 CO2(g) + 5 H20(1) A,H° -5779 kJ/mol Calculate the heat capacity of the calorimeter. heat capacity of calorimeter= orc J/C