A 58.1 g sample of quartz is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The quartz sample starts off at 87.4 °C and the temperature of the water starts off at 16.0 °C. When the temperature of the water stops changing it's 18.3 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of quartz according to this experiment. Be sure your answer is rounded to the correct number of significant digits. J 0- g. °C X thermometer. insulated container water sample. a calorimeter
A 58.1 g sample of quartz is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The quartz sample starts off at 87.4 °C and the temperature of the water starts off at 16.0 °C. When the temperature of the water stops changing it's 18.3 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of quartz according to this experiment. Be sure your answer is rounded to the correct number of significant digits. J 0- g. °C X thermometer. insulated container water sample. a calorimeter
Chemistry
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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
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![**Calorimetry Experiment: Calculating Specific Heat Capacity of Quartz**
**Experiment Details:**
A 58.1 g sample of quartz is placed into a calorimeter, as shown in the accompanying diagram, which contains 300.0 g of water. Initially, the quartz sample has a temperature of 87.4 °C, while the water starts at 16.0 °C. The temperature of the water changes until it stabilizes at 18.3 °C. Throughout the experiment, pressure is maintained at 1 atm.
**Task:**
Calculate the specific heat capacity of quartz based on this experiment. Ensure your answer is rounded to the appropriate number of significant figures.
**Diagram Explanation:**
The diagram shows the setup of the calorimetry experiment:
- **Thermometer**: Used to measure the temperature of the water.
- **Insulated Container**: Ensures minimal heat exchange with the surroundings.
- **Water**: 300.0 g, initial temperature 16.0 °C.
- **Sample**: Quartz, 58.1 g, initial temperature 87.4 °C.
- The final temperature of the water is 18.3 °C.
**Calculation:**
The specific heat capacity (\(c\)) of quartz can be determined using the heat exchange formula, where heat lost by quartz is equal to heat gained by water. The specific heat capacity of water is generally known.
\[
\text{Heat lost by quartz} = \text{Heat gained by water}
\]
\[
(m \cdot c \cdot \Delta T)_{\text{quartz}} = (m \cdot c \cdot \Delta T)_{\text{water}}
\]
Round your answer appropriately to reflect the precision of the given data.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd11077d3-f0b7-424b-830f-d72f05e11bec%2F3f8fde56-d280-406a-9476-80e837c3dcd0%2Fc0qeb88_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Calorimetry Experiment: Calculating Specific Heat Capacity of Quartz**
**Experiment Details:**
A 58.1 g sample of quartz is placed into a calorimeter, as shown in the accompanying diagram, which contains 300.0 g of water. Initially, the quartz sample has a temperature of 87.4 °C, while the water starts at 16.0 °C. The temperature of the water changes until it stabilizes at 18.3 °C. Throughout the experiment, pressure is maintained at 1 atm.
**Task:**
Calculate the specific heat capacity of quartz based on this experiment. Ensure your answer is rounded to the appropriate number of significant figures.
**Diagram Explanation:**
The diagram shows the setup of the calorimetry experiment:
- **Thermometer**: Used to measure the temperature of the water.
- **Insulated Container**: Ensures minimal heat exchange with the surroundings.
- **Water**: 300.0 g, initial temperature 16.0 °C.
- **Sample**: Quartz, 58.1 g, initial temperature 87.4 °C.
- The final temperature of the water is 18.3 °C.
**Calculation:**
The specific heat capacity (\(c\)) of quartz can be determined using the heat exchange formula, where heat lost by quartz is equal to heat gained by water. The specific heat capacity of water is generally known.
\[
\text{Heat lost by quartz} = \text{Heat gained by water}
\]
\[
(m \cdot c \cdot \Delta T)_{\text{quartz}} = (m \cdot c \cdot \Delta T)_{\text{water}}
\]
Round your answer appropriately to reflect the precision of the given data.
Expert Solution
Step 1: Law of conservation of energy
Answer:
According to law of conservation of energy, energy can't be destroyed or created, it can only be converted from one form into another. That's why heat lost by hotter object (quartz) will be equal to heat gained by colder substance (water).
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