A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuelsand the energy content of foods.Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of thecalorimeter. This is known as calibrating the calorimeter.In the laboratory a student burns a 0.578 g sample of nonanedioic acid (C9H1604) in a bomb calorimeter containing 1020 g of water. The temperature increases from 24.90°C to 27.80°C. The heatcapacity of water is4.184 J/(g °C).The molar heat of combustion is -4774 kJ per mole of nonanedioic acid.C9H16 O4(s)+1102(g) → 9CO2 (g) + 8H2O(l) + Energy

Answered: A bomb calorimeter, or constant volume…

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

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 112AE: In a bomb calorimeter, the reaction vessel is surrounded by water that must be added for each...

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What mass of acetylene, C2H2(g), must be burned to produce 3420 kJ of heat, given that its enthalpy of combustion is 1301 kJ/mol? Compare this with the answer to Exercise 5.91 and determine which substance produces more heat per gram.
Chlorine dioxide, ClO2, is a reddish yellow gas used in bleaching paper pulp. The average speed of a ClO2 molecule at 25C is 306 m/s. What is the kinetic energy (in joules) of a ClO2 molecule moving at this speed?
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Hypothetical elements A2 and B2 react according to the following equation, forming the compound AB. A2(aq)+B2(aq)2AB(aq);H=+271kJ/mol If solutions A2(aq) and B2(aq), starting at the same temperature, are mixed in a coffee-cup calorimeter, the reaction that occurs is a exothermic, and the temperature of the resulting solution rises. b endothermic, and the temperature of the resulting solution rises. c endothermic, and the temperature of the resulting solution falls. d exothermic, and the temperature of the resulting solution falls. e exothermic or endothermic, depending on the original and final temperatures.
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A sample of natural gas is 80.0% CH4 and 20.0% C2H6 by mass. What is the heat from the combustion of 1.00 g of this mixture? Assume the products are CO2(g) and H2O(l).
How much heat is absorbed by a 44.7-g piece of leadwhen its temperature increases by 65.4°C?
The combustion of 1.00 mol liquid methyl alcohol (CH3OH) in excess oxygen is exothermic, giving 727 kJ of heat. (a) Write the thermochemical equation for this reaction. (b) Calculate the enthalpy change that accompanies the burning 10.0 g methanol. (c) Compare this with the amount of heat produced by 10.0 g octane, C8H18, a component of gasoline (see Exercise 5.41).

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