Try Again Your answer is incorrect. • Row 2: Your answer is wrong. In addition to checking your math, check that you used the right data and DID NOT round any intermediate calculations. • Row 3: Your answer is wrong. In addition to checking your math, check that you used the right data and DID NOT round any intermediate calculations. A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). thermometer stirrer First, a 6.000 g tablet of benzoic acid (CH,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 insulati observed to rise from 15.00 °C to 45.70 °C over a time of 13.8 minutes. Next, 4.490 g of ethanol (C,H,OH) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 15.00 °C to 40.60 °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. C,H;OH(1) + 30,(8) - 2 CO,(g) + 3 H,O(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 mat published values for this reaction. O exothermic 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. -159.9 kJ kJ -63832 mol Calculate the reaction enthalpy AH per mole of C,H,OH. rxn
Try Again Your answer is incorrect. • Row 2: Your answer is wrong. In addition to checking your math, check that you used the right data and DID NOT round any intermediate calculations. • Row 3: Your answer is wrong. In addition to checking your math, check that you used the right data and DID NOT round any intermediate calculations. A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). thermometer stirrer First, a 6.000 g tablet of benzoic acid (CH,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 insulati observed to rise from 15.00 °C to 45.70 °C over a time of 13.8 minutes. Next, 4.490 g of ethanol (C,H,OH) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 15.00 °C to 40.60 °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. C,H;OH(1) + 30,(8) - 2 CO,(g) + 3 H,O(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 mat published values for this reaction. O exothermic 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. -159.9 kJ kJ -63832 mol Calculate the reaction enthalpy AH per mole of C,H,OH. rxn
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
Related questions
Question
plz use correct sig figs and make sure the answer is correct. i cant find a good example for this one
Transcribed Image Text:Try Again
Your answer is incorrect.
• Row 2: Your answer is wrong. In addition to checking your math, check that you used the right data and DID NOT round any intermediate calculations.
• Row 3: Your answer is wrong. In addition to checking your math, check that you used the right data and DID NOT round any intermediate calculations.
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch
at right).
thermometer
stirrer
First, a 6.000 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
insulatic
observed to rise from 15.00 °C to 45.70 °C over a time of 13.8 minutes.
Next, 4.490 g
ethanol (C,H;OH) :
are put into the "bomb" and similarly completely burned in an excess of
oxygen. This time the temperature of the water rises from 15.00 °C to 40.60 °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.
C,H,OH(1) + 3 02(g)
2 CO,(g) + 3 H,O(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 mato
published values for this reaction.
O exothermic
Ox10
Is this reaction exothermic, endothermic, or neither?
endothermic
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.
- 159.9 kJ
kJ
-63832
mol
Calculate the reaction enthalpy AH,
per mole of C,H,OH.
rxn
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 8 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemical-engineering and related others by exploring similar questions and additional content below.Recommended textbooks for you
Introduction to Chemical Engineering Thermodynami…
Chemical Engineering
ISBN:
9781259696527
Author:
J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:
McGraw-Hill Education
Elementary Principles of Chemical Processes, Bind…
Chemical Engineering
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
Elements of Chemical Reaction Engineering (5th Ed…
Chemical Engineering
ISBN:
9780133887518
Author:
H. Scott Fogler
Publisher:
Prentice Hall
Introduction to Chemical Engineering Thermodynami…
Chemical Engineering
ISBN:
9781259696527
Author:
J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:
McGraw-Hill Education
Elementary Principles of Chemical Processes, Bind…
Chemical Engineering
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
Elements of Chemical Reaction Engineering (5th Ed…
Chemical Engineering
ISBN:
9780133887518
Author:
H. Scott Fogler
Publisher:
Prentice Hall
Industrial Plastics: Theory and Applications
Chemical Engineering
ISBN:
9781285061238
Author:
Lokensgard, Erik
Publisher:
Delmar Cengage Learning
Unit Operations of Chemical Engineering
Chemical Engineering
ISBN:
9780072848236
Author:
Warren McCabe, Julian C. Smith, Peter Harriott
Publisher:
McGraw-Hill Companies, The