A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water (see sketch at right). First, a 7.000 g tablet of benzoic acid (CH-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 19.00 °C to 54.07 °C over a time of 14.3 minutes. Next, 4.940 g of acetylene (C₂H₂) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 19.00 °C to 63.23 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about 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 AHxn per mole of H₂O. O exothermic O endothermic O neither 0 2C₂H₂(g) + 50₂(g) 4CO₂(g) + 2 H₂O(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. KJ kJ stirrer mol thermometer - chemical reaction "bomb" A "bomb" calorimeter. water insulation S

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...
icon
Related questions
icon
Concept explainers
Question
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water (see sketch at
right).
First, a 7.000 g tablet of benzoic acid (C6H₂CO₂H) 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 19.00 °C to 54.07 °C over a time of 14.3 minutes.
Next, 4.940 g of acetylene (C₂H₂) are put into the "bomb" and similarly completely burned in an excess of oxygen.
This time the temperature of the water rises from 19.00 °C to 63.23 °C.
Use this information, and any other information you need from the ALEKS Data resource, to answer the questions
below about this reaction:
+
502 (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 H₂O.
O exothermic
O endothermic
O neither
2C₂H₂(g)
4CO₂(g) + 2 H₂O(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.
kJ
stirrer
kJ
mol
"bomb"
thermometer
chemical reaction
A "bomb" calorimeter.
water
0x0
insulation
Transcribed Image Text:A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water (see sketch at right). First, a 7.000 g tablet of benzoic acid (C6H₂CO₂H) 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 19.00 °C to 54.07 °C over a time of 14.3 minutes. Next, 4.940 g of acetylene (C₂H₂) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 19.00 °C to 63.23 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: + 502 (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 H₂O. O exothermic O endothermic O neither 2C₂H₂(g) 4CO₂(g) + 2 H₂O(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. kJ stirrer kJ mol "bomb" thermometer chemical reaction A "bomb" calorimeter. water 0x0 insulation
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 4 steps with 2 images

Blurred answer
Knowledge Booster
Thermochemistry
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.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY