A 48.70 g sample of pure copper is heated in a test tube to 99.40 °C. The copper sample is the transien water. The water temperature in the calorimeter rises from 24.43 °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) Initial temperature of water (°C) Final temperature of water (°C) Specific heat of water Specific heat of copper g-°C Value 48.70 99.40 61.04 24.43 29.10 J g-°C 4.184 0.385 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. Heat capacity of calorimeter= S
A 48.70 g sample of pure copper is heated in a test tube to 99.40 °C. The copper sample is the transien water. The water temperature in the calorimeter rises from 24.43 °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) Initial temperature of water (°C) Final temperature of water (°C) Specific heat of water Specific heat of copper g-°C Value 48.70 99.40 61.04 24.43 29.10 J g-°C 4.184 0.385 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. Heat capacity of calorimeter= S
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
Chapter6: Thermochemistry
Section: Chapter Questions
Problem 112AE: In a bomb calorimeter, the reaction vessel is surrounded by water that must be added for each...
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![A 48.70 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 24.43 °C to 29.10 °C. The collected data are listed in the following table.
| Measurement or constant | Value |
|------------------------------|-----------|
| Mass of pure copper (g) | 48.70 |
| Temperature of copper (°C) | 99.40 |
| Mass of water (g) | 61.04 |
| Initial temperature of water (°C) | 24.43 |
| Final temperature of water (°C) | 29.10 |
| Specific heat of water (J g⁻¹ °C⁻¹) | 4.184 |
| Specific heat of copper (J g⁻¹ °C⁻¹) | 0.385 |
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.
Heat capacity of calorimeter = __________ J/°C](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F11fddf9f-a89a-44ba-8382-9c550e4fed12%2Fbc3be3ad-ce1c-42d0-adc2-9667831651b4%2F765ha7w_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A 48.70 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 24.43 °C to 29.10 °C. The collected data are listed in the following table.
| Measurement or constant | Value |
|------------------------------|-----------|
| Mass of pure copper (g) | 48.70 |
| Temperature of copper (°C) | 99.40 |
| Mass of water (g) | 61.04 |
| Initial temperature of water (°C) | 24.43 |
| Final temperature of water (°C) | 29.10 |
| Specific heat of water (J g⁻¹ °C⁻¹) | 4.184 |
| Specific heat of copper (J g⁻¹ °C⁻¹) | 0.385 |
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.
Heat capacity of calorimeter = __________ J/°C
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