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
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
- Suggest some ways in which the calorimeter or lab protocol could be improved to have lower percentage of errors.
![**Data Table 2**
| | 5g CaCl₂ | 10g CaCl₂ | 15g CaCl₂ | 5g NH₄Cl | 10g NH₄Cl | 15g NH₄Cl |
|----------------------|----------|-----------|-----------|----------|-----------|-----------|
| Mass of water (g) | 100 | 100 | 100 | 100 | 100 | 100 |
| Mass of salt (g) | 5.0 | 10.04 | 15.0 | 5.0 | 10.02 | 15.0 |
| Moles of salt \[g x mol/g\] | 0.045 | 0.090 | 0.135 | 0.093 | 0.187 | 0.280 |
| Initial Temperature (°C) | 23 | 23 | 23 | 23 | 23 | 23 |
| Final Temperature (°C) | 29 | 37 | 42 | 19 | 15 | 12 |
| Change in Temperature (°C) \[ΔT = Tf - Ti\] | 6 | 14 | 19 | -4 | -8 | -11 |
| Heat absorbed by the solution (J) \[qₓ = \[-q⁰ₓ = -mcΔT\]\] | -125.5 | -585.8 | -1192.4 | 83.7 | 335.4 | 690.4 |
| Heat Capacity of the Calorimeter (J/°C) \[C\] | 418.4 | 418.4 | 418.4 | 418.4 | 418.4 | 418.4 |
| Heat absorbed by the calorimeter (J) \[qₑ = C x ΔT\] | 2510.4 | 5857.6 | 7949.6 | 1673.6 | 3347.2 | 4602.4 |
| Enthalpy of solution](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa4431abc-b804-490c-9182-b6054ed16985%2F2679d797-b340-4789-81ec-8cd742885456%2Fl9idk2j.jpeg&w=3840&q=75)
Transcribed Image Text:**Data Table 2**
| | 5g CaCl₂ | 10g CaCl₂ | 15g CaCl₂ | 5g NH₄Cl | 10g NH₄Cl | 15g NH₄Cl |
|----------------------|----------|-----------|-----------|----------|-----------|-----------|
| Mass of water (g) | 100 | 100 | 100 | 100 | 100 | 100 |
| Mass of salt (g) | 5.0 | 10.04 | 15.0 | 5.0 | 10.02 | 15.0 |
| Moles of salt \[g x mol/g\] | 0.045 | 0.090 | 0.135 | 0.093 | 0.187 | 0.280 |
| Initial Temperature (°C) | 23 | 23 | 23 | 23 | 23 | 23 |
| Final Temperature (°C) | 29 | 37 | 42 | 19 | 15 | 12 |
| Change in Temperature (°C) \[ΔT = Tf - Ti\] | 6 | 14 | 19 | -4 | -8 | -11 |
| Heat absorbed by the solution (J) \[qₓ = \[-q⁰ₓ = -mcΔT\]\] | -125.5 | -585.8 | -1192.4 | 83.7 | 335.4 | 690.4 |
| Heat Capacity of the Calorimeter (J/°C) \[C\] | 418.4 | 418.4 | 418.4 | 418.4 | 418.4 | 418.4 |
| Heat absorbed by the calorimeter (J) \[qₑ = C x ΔT\] | 2510.4 | 5857.6 | 7949.6 | 1673.6 | 3347.2 | 4602.4 |
| Enthalpy of solution
Transcribed Image Text:### Transcription for Educational Website
#### Data Table
| Mass (g) | CaCl₂ ΔT (°C) | NH₄Cl Mass (g) | NH₄Cl ΔT (°C) |
|----------|--------------|----------------|--------------|
| 5 | 6 | 5 | -4 |
| 10.04 | 14 | 10.02 | -8 |
| 15 | 19 | 15 | -11 |
#### Graph Descriptions
**Chart #1: Mass of CaCl₂ vs. ΔT**
- **X-axis:** Mass of CaCl₂ (in grams)
- **Y-axis:** Change in Temperature (ΔT, in °C)
- **Description:** The chart presents a linear relationship between the mass of calcium chloride (CaCl₂) and the change in temperature (ΔT).
- **Equation of the Line:** \( y = 1.3008x - 0.0251 \)
- **Coefficient of Determination (R²):** 0.9837
- **Observation:** As the mass of CaCl₂ increases, the change in temperature also increases, indicating a direct proportionality.
**Chart #2: Mass of NH₄Cl vs. ΔT**
- **X-axis:** Mass of NH₄Cl (in grams)
- **Y-axis:** Change in Temperature (ΔT, in °C)
- **Description:** This chart displays a linear inverse relationship between the mass of ammonium chloride (NH₄Cl) and the change in temperature (ΔT).
- **Equation of the Line:** \( y = -0.7001x - 0.6607 \)
- **Coefficient of Determination (R²):** 0.9936
- **Observation:** As the mass of NH₄Cl increases, the change in temperature decreases, reflecting an inverse proportionality and indicating an endothermic reaction.
#### Source
Data provided by © 2016 Carolina Biological Supply Company.
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
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