**Calorimetry Experiment: Heat of Reaction** In this experiment, 500 mL of a 1.00 M solution of CuSO₄ is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The initial temperature of both solutions is 20.2°C before mixing, and the temperature rises to 26.3°C after mixing. The heat capacity of the calorimeter is 12.1 J/K. The goal is to calculate the change in enthalpy (∆H) for the following chemical reaction: \[ \text{CuSO}_4(1 \text{ M}) + 2\text{KOH}(2 \text{ M}) \rightarrow \text{Cu(OH)}_2(s) + \text{K}_2\text{SO}_4(0.5 \text{ M}) \] Assume the specific heat and density of the solution after mixing are the same as those of pure water, and that volumes are additive. **Key Concepts:** - **Specific Heat Capacity:** The amount of heat required to raise the temperature of 1 gram of a substance by 1°C. - **Calorimetry:** The measurement of heat flow in a chemical reaction. - **Enthalpy Change (∆H):** Represents the heat absorbed or evolved during a reaction at constant pressure. **Procedure Overview:** 1. Mix CuSO₄ and KOH solutions in the calorimeter. 2. Measure the temperature change. 3. Calculate the heat absorbed or evolved using the formula: \[ q = m \cdot c \cdot \Delta T + C_{\text{calorimeter}} \cdot \Delta T \] where \( m \) is the mass of the solution, \( c \) is the specific heat capacity, \( \Delta T \) is the temperature change, and \( C_{\text{calorimeter}} \) is the calorimeter heat capacity. 4. Determine the enthalpy change per mole of reaction with the calculated heat and molarity of the solutions. **Understanding and Calculating ∆H:** - Use measured temperature change, volume, concentration, and specific heat to compute the heat involved in the reaction. - Apply stoichiometry of the reaction to relate the heat measurement to enthalpy. By understanding these methods, students can explore the energetic relationships within chemical systems and practice
**Calorimetry Experiment: Heat of Reaction** In this experiment, 500 mL of a 1.00 M solution of CuSO₄ is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The initial temperature of both solutions is 20.2°C before mixing, and the temperature rises to 26.3°C after mixing. The heat capacity of the calorimeter is 12.1 J/K. The goal is to calculate the change in enthalpy (∆H) for the following chemical reaction: \[ \text{CuSO}_4(1 \text{ M}) + 2\text{KOH}(2 \text{ M}) \rightarrow \text{Cu(OH)}_2(s) + \text{K}_2\text{SO}_4(0.5 \text{ M}) \] Assume the specific heat and density of the solution after mixing are the same as those of pure water, and that volumes are additive. **Key Concepts:** - **Specific Heat Capacity:** The amount of heat required to raise the temperature of 1 gram of a substance by 1°C. - **Calorimetry:** The measurement of heat flow in a chemical reaction. - **Enthalpy Change (∆H):** Represents the heat absorbed or evolved during a reaction at constant pressure. **Procedure Overview:** 1. Mix CuSO₄ and KOH solutions in the calorimeter. 2. Measure the temperature change. 3. Calculate the heat absorbed or evolved using the formula: \[ q = m \cdot c \cdot \Delta T + C_{\text{calorimeter}} \cdot \Delta T \] where \( m \) is the mass of the solution, \( c \) is the specific heat capacity, \( \Delta T \) is the temperature change, and \( C_{\text{calorimeter}} \) is the calorimeter heat capacity. 4. Determine the enthalpy change per mole of reaction with the calculated heat and molarity of the solutions. **Understanding and Calculating ∆H:** - Use measured temperature change, volume, concentration, and specific heat to compute the heat involved in the reaction. - Apply stoichiometry of the reaction to relate the heat measurement to enthalpy. By understanding these methods, students can explore the energetic relationships within chemical systems and practice
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
Question
Need help with #4
![**Calorimetry Experiment: Heat of Reaction**
In this experiment, 500 mL of a 1.00 M solution of CuSO₄ is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The initial temperature of both solutions is 20.2°C before mixing, and the temperature rises to 26.3°C after mixing. The heat capacity of the calorimeter is 12.1 J/K. The goal is to calculate the change in enthalpy (∆H) for the following chemical reaction:
\[ \text{CuSO}_4(1 \text{ M}) + 2\text{KOH}(2 \text{ M}) \rightarrow \text{Cu(OH)}_2(s) + \text{K}_2\text{SO}_4(0.5 \text{ M}) \]
Assume the specific heat and density of the solution after mixing are the same as those of pure water, and that volumes are additive.
**Key Concepts:**
- **Specific Heat Capacity:** The amount of heat required to raise the temperature of 1 gram of a substance by 1°C.
- **Calorimetry:** The measurement of heat flow in a chemical reaction.
- **Enthalpy Change (∆H):** Represents the heat absorbed or evolved during a reaction at constant pressure.
**Procedure Overview:**
1. Mix CuSO₄ and KOH solutions in the calorimeter.
2. Measure the temperature change.
3. Calculate the heat absorbed or evolved using the formula:
\[ q = m \cdot c \cdot \Delta T + C_{\text{calorimeter}} \cdot \Delta T \]
where \( m \) is the mass of the solution, \( c \) is the specific heat capacity, \( \Delta T \) is the temperature change, and \( C_{\text{calorimeter}} \) is the calorimeter heat capacity.
4. Determine the enthalpy change per mole of reaction with the calculated heat and molarity of the solutions.
**Understanding and Calculating ∆H:**
- Use measured temperature change, volume, concentration, and specific heat to compute the heat involved in the reaction.
- Apply stoichiometry of the reaction to relate the heat measurement to enthalpy.
By understanding these methods, students can explore the energetic relationships within chemical systems and practice](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7a86590d-c1f5-4894-93d9-46c435b15aa5%2F76d0fe49-e242-4dd3-b27c-9becd09f8334%2F9h41vj4.jpeg&w=3840&q=75)
Transcribed Image Text:**Calorimetry Experiment: Heat of Reaction**
In this experiment, 500 mL of a 1.00 M solution of CuSO₄ is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The initial temperature of both solutions is 20.2°C before mixing, and the temperature rises to 26.3°C after mixing. The heat capacity of the calorimeter is 12.1 J/K. The goal is to calculate the change in enthalpy (∆H) for the following chemical reaction:
\[ \text{CuSO}_4(1 \text{ M}) + 2\text{KOH}(2 \text{ M}) \rightarrow \text{Cu(OH)}_2(s) + \text{K}_2\text{SO}_4(0.5 \text{ M}) \]
Assume the specific heat and density of the solution after mixing are the same as those of pure water, and that volumes are additive.
**Key Concepts:**
- **Specific Heat Capacity:** The amount of heat required to raise the temperature of 1 gram of a substance by 1°C.
- **Calorimetry:** The measurement of heat flow in a chemical reaction.
- **Enthalpy Change (∆H):** Represents the heat absorbed or evolved during a reaction at constant pressure.
**Procedure Overview:**
1. Mix CuSO₄ and KOH solutions in the calorimeter.
2. Measure the temperature change.
3. Calculate the heat absorbed or evolved using the formula:
\[ q = m \cdot c \cdot \Delta T + C_{\text{calorimeter}} \cdot \Delta T \]
where \( m \) is the mass of the solution, \( c \) is the specific heat capacity, \( \Delta T \) is the temperature change, and \( C_{\text{calorimeter}} \) is the calorimeter heat capacity.
4. Determine the enthalpy change per mole of reaction with the calculated heat and molarity of the solutions.
**Understanding and Calculating ∆H:**
- Use measured temperature change, volume, concentration, and specific heat to compute the heat involved in the reaction.
- Apply stoichiometry of the reaction to relate the heat measurement to enthalpy.
By understanding these methods, students can explore the energetic relationships within chemical systems and practice
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 4 steps
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