A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). First, a 5.000 g tablet of benzoic acid (C6H5CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 17.00 °C to 41.54 °C over a time of 8.1 minutes. Next, 5.510 g of ethylene (C₂H4) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 17.00 °C to 63.77 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: C₂H4(g) + 30₂(g) → 2CO₂(g) + 2H₂O (8) Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. Calculate the reaction enthalpy AHxn per mole of CO₂. exothermic O endothermic Oneither kJ 0 kJ mol I stirrer 0 thermometer chemical reaction "bomb" A "bomb" calorimeter. water insulation.
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). First, a 5.000 g tablet of benzoic acid (C6H5CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 17.00 °C to 41.54 °C over a time of 8.1 minutes. Next, 5.510 g of ethylene (C₂H4) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 17.00 °C to 63.77 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: C₂H4(g) + 30₂(g) → 2CO₂(g) + 2H₂O (8) Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. Calculate the reaction enthalpy AHxn per mole of CO₂. exothermic O endothermic Oneither kJ 0 kJ mol I stirrer 0 thermometer chemical reaction "bomb" A "bomb" calorimeter. water insulation.
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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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
Transcribed Image Text:A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at
right).
First, a 5.000 g tablet of benzoic acid (C6H-CO₂H) is put into the "bomb" and burned completely in an excess of
oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is
observed to rise from 17.00 °C to 41.54 °C over a time of 8.1 minutes.
Next, 5.510 g of ethylene (C₂H4) are put into the "bomb" and similarly completely burned in an excess of oxygen.
This time the temperature of the water rises from 17.00 °C to 63.77 °C.
Use this information, and any other information you need from the ALEKS Data resource, to answer the questions
below about this reaction:
C₂H₂(g) + 30₂(g) → 2CO₂(g) + 2H₂O(g)
Is this reaction exothermic, endothermic, or neither?
If you said the reaction was exothermic or endothermic, calculate the amount of heat that was
released or absorbed by the reaction in the second experiment.
Calculate the reaction enthalpy AHxn per mole of CO₂.
exothermic
O endothermic
Oneither
KJ
0
kJ
mol
stirrer
0
thermometer
chemical reaction
"bomb"
"bomb" calorimeter.
water
insulation
match
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