A 50.10 g sample of pure copper is heated in a test tube to 99.40 °C. The copper sample is then transferred to a calorimeter containing 61.04 g of delonized water. The water temperature in the calorimeter rises from 24.51 °C to 29.10 °C. The collected data are listed in the following table. Measurement or constant Mass of pure copper (g) Temperature of copper (°C) Mass of water (g) Value 50.10 99.40 61.04 Initial temperature of water (°C) 24.51 Final temperature of water (°C) 29.10 Specific heat of water. (PPC) (PFC) Assuming that heat was transferred from the copper to the water and the calorimeter, determine the heat capacity of the calorimeter. Round your answer to 2 significant digits. Specific heat of copper 4.184 0.385
A 50.10 g sample of pure copper is heated in a test tube to 99.40 °C. The copper sample is then transferred to a calorimeter containing 61.04 g of delonized water. The water temperature in the calorimeter rises from 24.51 °C to 29.10 °C. The collected data are listed in the following table. Measurement or constant Mass of pure copper (g) Temperature of copper (°C) Mass of water (g) Value 50.10 99.40 61.04 Initial temperature of water (°C) 24.51 Final temperature of water (°C) 29.10 Specific heat of water. (PPC) (PFC) Assuming that heat was transferred from the copper to the water and the calorimeter, determine the heat capacity of the calorimeter. Round your answer to 2 significant digits. Specific heat of copper 4.184 0.385
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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![## Heat Capacity Calculation of a Calorimeter
A 50.10 g sample of pure copper is heated in a test tube to 99.40°C. The copper sample is then transferred to a calorimeter containing 61.04 g of deionized water. The water temperature in the calorimeter rises from 24.51°C to 29.10°C. The collected data are listed in the following table:
| Measurement or constant | Value |
|------------------------------|-----------|
| Mass of pure copper (g) | 50.10 |
| Temperature of copper (°C) | 99.40 |
| Mass of water (g) | 61.04 |
| Initial temperature of water (°C) | 24.51 |
| Final temperature of water (°C) | 29.10 |
| Specific heat of water (J/g·°C) | 4.184 |
| Specific heat of copper (J/g·°C) | 0.385 |
Assuming that heat was transferred from the copper to the water and the calorimeter, determine the heat capacity of the calorimeter.
### Calculation
To find the heat capacity of the calorimeter, you'll need to follow these steps:
1. Calculate the heat gained by the water:
\[
q_{\text{water}} = m_{\text{water}} \times c_{\text{water}} \times \Delta T_{\text{water}}
\]
Where:
- \( m_{\text{water}} \) is the mass of water
- \( c_{\text{water}} \) is the specific heat of water
- \( \Delta T_{\text{water}} \) is the change in the water temperature
2. Calculate the heat lost by the copper:
\[
q_{\text{copper}} = m_{\text{copper}} \times c_{\text{copper}} \times \Delta T_{\text{copper}}
\]
Where:
- \( m_{\text{copper}} \) is the mass of copper
- \( c_{\text{copper}} \) is the specific heat of copper
- \( \Delta T_{\text{copper}} \) is the change in the copper temperature
3. The heat gained by the water and calorimeter must equal](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F11fddf9f-a89a-44ba-8382-9c550e4fed12%2Fdf9b2e83-23fd-4111-9a66-42ef57eb1fd6%2Fqgjnxor_processed.jpeg&w=3840&q=75)
Transcribed Image Text:## Heat Capacity Calculation of a Calorimeter
A 50.10 g sample of pure copper is heated in a test tube to 99.40°C. The copper sample is then transferred to a calorimeter containing 61.04 g of deionized water. The water temperature in the calorimeter rises from 24.51°C to 29.10°C. The collected data are listed in the following table:
| Measurement or constant | Value |
|------------------------------|-----------|
| Mass of pure copper (g) | 50.10 |
| Temperature of copper (°C) | 99.40 |
| Mass of water (g) | 61.04 |
| Initial temperature of water (°C) | 24.51 |
| Final temperature of water (°C) | 29.10 |
| Specific heat of water (J/g·°C) | 4.184 |
| Specific heat of copper (J/g·°C) | 0.385 |
Assuming that heat was transferred from the copper to the water and the calorimeter, determine the heat capacity of the calorimeter.
### Calculation
To find the heat capacity of the calorimeter, you'll need to follow these steps:
1. Calculate the heat gained by the water:
\[
q_{\text{water}} = m_{\text{water}} \times c_{\text{water}} \times \Delta T_{\text{water}}
\]
Where:
- \( m_{\text{water}} \) is the mass of water
- \( c_{\text{water}} \) is the specific heat of water
- \( \Delta T_{\text{water}} \) is the change in the water temperature
2. Calculate the heat lost by the copper:
\[
q_{\text{copper}} = m_{\text{copper}} \times c_{\text{copper}} \times \Delta T_{\text{copper}}
\]
Where:
- \( m_{\text{copper}} \) is the mass of copper
- \( c_{\text{copper}} \) is the specific heat of copper
- \( \Delta T_{\text{copper}} \) is the change in the copper temperature
3. The heat gained by the water and calorimeter must equal
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