Next, 4.490 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 12.00 °C to 52.29 °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? C₂H₂(g) + 30₂(g) → 2CO₂(g) + 2H₂O(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 exac published values for this reaction. 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 C₂H4. exothermic endothermic neither ☐ kJ chemical reaction kJ mol "bomb" A "bomb" calorimeter. X
Next, 4.490 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 12.00 °C to 52.29 °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? C₂H₂(g) + 30₂(g) → 2CO₂(g) + 2H₂O(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 exac published values for this reaction. 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 C₂H4. exothermic endothermic neither ☐ kJ chemical reaction kJ mol "bomb" A "bomb" calorimeter. X
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...
Related questions
Concept explainers
Types of Chemical Bonds
The attractive force which has the ability of holding various constituent elements like atoms, ions, molecules, etc. together in different chemical species is termed as a chemical bond. Chemical compounds are dependent on the strength of chemical bonds between its constituents. Stronger the chemical bond, more will be the stability in the chemical compounds. Hence, it can be said that bonding defines the stability of chemical compounds.
Polarizability In Organic Chemistry
Polarizability refers to the ability of an atom/molecule to distort the electron cloud of neighboring species towards itself and the process of distortion of electron cloud is known as polarization.
Coordinate Covalent Bonds
A coordinate covalent bond is also known as a dative bond, which is a type of covalent bond. It is formed between two atoms, where the two electrons required to form the bond come from the same atom resulting in a semi-polar bond. The study of coordinate covalent bond or dative bond is important to know about the special type of bonding that leads to different properties. Since covalent compounds are non-polar whereas coordinate bonds results always in polar compounds due to charge separation.
Question
![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 \((C_6H_5CO_2H)\) 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 12.00 °C to 45.56 °C over a time of 7.6 minutes.
Next, 4.490 g of ethylene \((C_2H_4)\) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 12.00 °C to 52.29 °C.
Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction:
\[
C_2H_4 (g) + 3O_2 (g) \rightarrow 2CO_2 (g) + 2H_2O (g)
\]
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.
1. Is this reaction exothermic, endothermic, or neither?
- Exothermic
- Endothermic
- Neither
2. 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
3. Calculate the reaction enthalpy \(\Delta H_{rxn}\) per mole of \(C_2H_4\).
[ ] kJ/mol
**Diagram Explanation:**
The diagram shows a "bomb" calorimeter, consisting of the following components:
- **Thermometer:** Measures the temperature change of the water.
- **Stirrer:** Ensures uniform distribution of heat.
- **Water:** Absorbs the heat released during the reaction.
- **Insulation:** Minimizes heat loss to the surroundings.
- **Bomb:** Contains the chemical](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F439811cd-3522-4321-811e-10b69707975d%2F307d9b5b-7d74-4fd2-989f-eecf36fa9708%2F550mf02_processed.jpeg&w=3840&q=75)
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 \((C_6H_5CO_2H)\) 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 12.00 °C to 45.56 °C over a time of 7.6 minutes.
Next, 4.490 g of ethylene \((C_2H_4)\) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 12.00 °C to 52.29 °C.
Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction:
\[
C_2H_4 (g) + 3O_2 (g) \rightarrow 2CO_2 (g) + 2H_2O (g)
\]
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.
1. Is this reaction exothermic, endothermic, or neither?
- Exothermic
- Endothermic
- Neither
2. 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
3. Calculate the reaction enthalpy \(\Delta H_{rxn}\) per mole of \(C_2H_4\).
[ ] kJ/mol
**Diagram Explanation:**
The diagram shows a "bomb" calorimeter, consisting of the following components:
- **Thermometer:** Measures the temperature change of the water.
- **Stirrer:** Ensures uniform distribution of heat.
- **Water:** Absorbs the heat released during the reaction.
- **Insulation:** Minimizes heat loss to the surroundings.
- **Bomb:** Contains the chemical
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 3 steps with 2 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
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY