Mass of aluminum 16.27 g Initial temperature of Al Volume of water 83.85°C 51.8 mL Initial temperature of water Final water temperature 20.30°C 23.90°C Density of water 1.00 mL Specific heat of water J 4.184 g• °C Calorimeter constant 22.44 A student adds a heated sample of pure aluminum metal to a Styrofoam coffee cup calorimeter containing deionized water. Use the collected data to answer the following questions. (a) Assuming that heat was transferred from the aluminum to the water and the calorimeter, determine the specific heat of aluminum. J Specific heat of AlI= | g. °C J (b) The actual specific heat of aluminum is 0.900 Calculate the percent error for the g. °C experimentally determined specific heat. Percent error %
Mass of aluminum 16.27 g Initial temperature of Al Volume of water 83.85°C 51.8 mL Initial temperature of water Final water temperature 20.30°C 23.90°C Density of water 1.00 mL Specific heat of water J 4.184 g• °C Calorimeter constant 22.44 A student adds a heated sample of pure aluminum metal to a Styrofoam coffee cup calorimeter containing deionized water. Use the collected data to answer the following questions. (a) Assuming that heat was transferred from the aluminum to the water and the calorimeter, determine the specific heat of aluminum. J Specific heat of AlI= | g. °C J (b) The actual specific heat of aluminum is 0.900 Calculate the percent error for the g. °C experimentally determined specific heat. Percent error %
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...
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![**Calorimetry Experiment with Aluminum and Water**
**Experimental Data:**
- **Mass of aluminum:** 16.27 g
- **Initial temperature of Al:** 83.85°C
- **Volume of water:** 51.8 mL
- **Initial temperature of water:** 20.30°C
- **Final water temperature:** 23.90°C
- **Density of water:** 1.00 g/mL
- **Specific heat of water:** 4.184 J/g°C
- **Calorimeter constant:** 22.44 J/°C
**Procedure:**
A student adds a heated sample of pure aluminum metal to a Styrofoam coffee cup calorimeter containing deionized water. Use the collected data to answer the following questions:
**Questions:**
(a) Assuming that heat was transferred from the aluminum to the water and the calorimeter, determine the specific heat of aluminum.
\[ \text{Specific heat of Al} = \boxed{\phantom{\frac{J}{g \cdot °C}}} \]
(b) The actual specific heat of aluminum is 0.900 J/g°C. Calculate the percent error for the experimentally determined specific heat.
\[ \text{Percent error} = \boxed{\phantom{\%\%}} \]
**Explanation:**
This experiment aims to determine the specific heat of aluminum through calorimetry. By measuring the temperature changes in water, we can calculate the heat exchange and thus infer the specific heat capacity of the aluminum sample. The percent error will help in understanding the accuracy of the experimentally determined value compared to the known specific heat of aluminum.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff2706e7c-aa15-40ae-946e-efc678bb7f7c%2Fc1998cea-f293-4a91-baf2-11d127edbc07%2Fm3yiwp_processed.png&w=3840&q=75)
Transcribed Image Text:**Calorimetry Experiment with Aluminum and Water**
**Experimental Data:**
- **Mass of aluminum:** 16.27 g
- **Initial temperature of Al:** 83.85°C
- **Volume of water:** 51.8 mL
- **Initial temperature of water:** 20.30°C
- **Final water temperature:** 23.90°C
- **Density of water:** 1.00 g/mL
- **Specific heat of water:** 4.184 J/g°C
- **Calorimeter constant:** 22.44 J/°C
**Procedure:**
A student adds a heated sample of pure aluminum metal to a Styrofoam coffee cup calorimeter containing deionized water. Use the collected data to answer the following questions:
**Questions:**
(a) Assuming that heat was transferred from the aluminum to the water and the calorimeter, determine the specific heat of aluminum.
\[ \text{Specific heat of Al} = \boxed{\phantom{\frac{J}{g \cdot °C}}} \]
(b) The actual specific heat of aluminum is 0.900 J/g°C. Calculate the percent error for the experimentally determined specific heat.
\[ \text{Percent error} = \boxed{\phantom{\%\%}} \]
**Explanation:**
This experiment aims to determine the specific heat of aluminum through calorimetry. By measuring the temperature changes in water, we can calculate the heat exchange and thus infer the specific heat capacity of the aluminum sample. The percent error will help in understanding the accuracy of the experimentally determined value compared to the known specific heat of aluminum.
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