A student Tuns twoexpermemts WitIT a Constant volume DOID CaloImeter CoTmta ng T1J00. g ur vwater (see SKettn at thermometer right). stirrer First, a 6.500 g tablet of benzoic acid (C,H,CO,H) is put into the "bomb" and burned completely in an excess of wate oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed ins to rise from 16.00 °C to 39.39 °C over a time of 9.6 minutes. Next, 5.940 g of acetylene (C,H,) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 16.00 °C to 52.65 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H, (g) + 50,(g) → 4CO,(g) + 2H,0 (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 ma published values for this reaction. O exothermic Oxto Is this reaction exothermic, endothermic, or neither? O endothermic O 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. kJ Calculate the reaction enthalpy AH per mole of C,H,. rxn
A student Tuns twoexpermemts WitIT a Constant volume DOID CaloImeter CoTmta ng T1J00. g ur vwater (see SKettn at thermometer right). stirrer First, a 6.500 g tablet of benzoic acid (C,H,CO,H) is put into the "bomb" and burned completely in an excess of wate oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed ins to rise from 16.00 °C to 39.39 °C over a time of 9.6 minutes. Next, 5.940 g of acetylene (C,H,) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 16.00 °C to 52.65 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H, (g) + 50,(g) → 4CO,(g) + 2H,0 (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 ma published values for this reaction. O exothermic Oxto Is this reaction exothermic, endothermic, or neither? O endothermic O 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. kJ Calculate the reaction enthalpy AH per mole of C,H,. rxn
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section: Chapter Questions
Problem 89QRT
Related questions
Concept explainers
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:thermometer
right).
stirrer
First, a 6.500 g tablet of benzoic acid (C,H,CO,H) is put into the "bomb" and burned completely in an excess of
water
oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed
insulation
to rise from 16.00 °C to 39.39 °C over a time of 9.6 minutes.
Next, 5.940 g of acetylene (C,H,)
are put into the "bomb" and similarly completely burned in an excess of oxygen.
This time the temperature of the water rises from 16.00 °C to 52.65 °C.
chemical reaction
"bomb"
Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below
about this reaction:
A "bomb" calorimeter.
2C,H, (g) + 50,(g)
4CO,(g) + 2H,0 (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.
exothermic
Is this reaction exothermic, endothermic, or neither?
endothermic
neither
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.
If
||kJ
kJ
Calculate the reaction enthalpy AH
per mole of C,H,.
U mol
rxn
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 3 steps with 3 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:
9781337399425
Author:
Steven S. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:
9781337399425
Author:
Steven S. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning