What is the key equation used in calorimetry experiments?

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
Question
**Title: Key Equation Used in Calorimetry Experiments**

**Question:** What is the key equation used in calorimetry experiments?

**Options:**
1. \( d = \frac{m}{V} \)
2. \( q_{\text{rxn}} = -q_{\text{cal}} \)
3. At endpoint, mol acid = mol base
4. \( A = \epsilon b C \)

**Explanation:**

1. **Option 1: \( d = \frac{m}{V} \)**
   - This equation is used to calculate the density of a substance, where \( d \) is density, \( m \) is mass, and \( V \) is volume.
   
2. **Option 2: \( q_{\text{rxn}} = -q_{\text{cal}} \)**
   - This is the key equation used in calorimetry. It states that the heat of the reaction (\( q_{\text{rxn}} \)) is equal to the negative of the heat absorbed by the calorimeter (\( q_{\text{cal}} \)). This principle is based on the law of conservation of energy, implying that the energy lost by the system must be gained by the surroundings.

3. **Option 3: At endpoint, mol acid = mol base**
   - This statement is relevant to titration experiments and not specific to calorimetry. It indicates that at the endpoint of a titration, the amount of moles of acid equals the amount of moles of base.

4. **Option 4: \( A = \epsilon b C \)**
   - This equation is known as Beer's Law in spectroscopy, where \( A \) is absorbance, \( \epsilon \) is molar absorptivity, \( b \) is path length, and \( C \) is concentration.

**Correct Answer:**
- The correct answer is **Option 2: \( q_{\text{rxn}} = -q_{\text{cal}} \)**.

This equation is essential for understanding and calculating the energy changes occurring during chemical reactions in calorimetry experiments.
Transcribed Image Text:**Title: Key Equation Used in Calorimetry Experiments** **Question:** What is the key equation used in calorimetry experiments? **Options:** 1. \( d = \frac{m}{V} \) 2. \( q_{\text{rxn}} = -q_{\text{cal}} \) 3. At endpoint, mol acid = mol base 4. \( A = \epsilon b C \) **Explanation:** 1. **Option 1: \( d = \frac{m}{V} \)** - This equation is used to calculate the density of a substance, where \( d \) is density, \( m \) is mass, and \( V \) is volume. 2. **Option 2: \( q_{\text{rxn}} = -q_{\text{cal}} \)** - This is the key equation used in calorimetry. It states that the heat of the reaction (\( q_{\text{rxn}} \)) is equal to the negative of the heat absorbed by the calorimeter (\( q_{\text{cal}} \)). This principle is based on the law of conservation of energy, implying that the energy lost by the system must be gained by the surroundings. 3. **Option 3: At endpoint, mol acid = mol base** - This statement is relevant to titration experiments and not specific to calorimetry. It indicates that at the endpoint of a titration, the amount of moles of acid equals the amount of moles of base. 4. **Option 4: \( A = \epsilon b C \)** - This equation is known as Beer's Law in spectroscopy, where \( A \) is absorbance, \( \epsilon \) is molar absorptivity, \( b \) is path length, and \( C \) is concentration. **Correct Answer:** - The correct answer is **Option 2: \( q_{\text{rxn}} = -q_{\text{cal}} \)**. This equation is essential for understanding and calculating the energy changes occurring during chemical reactions in calorimetry experiments.
Expert Solution
steps

Step by step

Solved in 2 steps

Blurred answer
Knowledge Booster
Thermodynamics
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
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