A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). First, a 6.000 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 21.00 °C to 51.70 °C over a time of 13.6 minutes. Next, 5.850 g of ethanol (C₂H5OH) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 21.00 °C to 54.35 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: C₂H₂OH(1) + 30₂(g) → 2CO₂(g) + 3H₂O(g) Is this reaction exothermic, endothermic, or neither? stirrer O exothermic O endothermic O neither 0 thermometer chemical reaction "bomb" A "bomb" calorimeter. Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values you calculate may not exactly match published values for this reaction. water X insulation S
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). First, a 6.000 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 21.00 °C to 51.70 °C over a time of 13.6 minutes. Next, 5.850 g of ethanol (C₂H5OH) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 21.00 °C to 54.35 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: C₂H₂OH(1) + 30₂(g) → 2CO₂(g) + 3H₂O(g) Is this reaction exothermic, endothermic, or neither? stirrer O exothermic O endothermic O neither 0 thermometer chemical reaction "bomb" A "bomb" calorimeter. Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values you calculate may not exactly match published values for this reaction. water X insulation S
Chemistry for Engineering Students
3rd Edition
ISBN:9781285199023
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter9: Energy And Chemistry
Section: Chapter Questions
Problem 9.79PAE: A student performing a calorimetry experiment combined 100.0 ml. of 0.50 M HCI and 100.0 ml. of 0.50...
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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
Please help with the following, make sure your asner is correct with proper signs 100%, pls and thank you
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 6.000 g tablet of benzoic acid (CH₂CO₂H) is put into the "bomb" and burned completely in an excess of
5
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 21.00 °C to 51.70 °C over a time of 13.6 minutes.
Next, 5.850 g of ethanol (C₂H5OH) are put into the "bomb" and similarly completely burned in an excess of oxygen.
This time the temperature of the water rises from 21.00 °C to 54.35 °C.
Use this information, and any other information you need from the ALEKS Data resource, to answer the questions
below about this reaction:
C₂H₂OH(1) + 30₂ (g) 2CO₂(g) + 3 H₂O(g)
2
Is this reaction exothermic, endothermic, or neither?
exothermic
endothermic
stirrer
neither
thermometer
chemical reaction
Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits.
Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values you calculate may not exactly match
published values for this reaction.
"bomb"
A "bomb" calorimeter.
x10
water
X
insulation
Ś
Transcribed Image Text:C₂H₂OH(1) + 302₂(g) 2CO₂(g) + 3H₂O(g)
Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits.
Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values you calculate may not exactly match
published values for this reaction.
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 ΔΗ per mole of H₂O.
rxn
0
exothermic
endothermic
neither
kJ
kJ
mol
x10
X
Ś
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