3.) An iron bar with a mass of 869 g cools from 94.0 °C to 5.0 °C. Calculate the heat released (in kilojoules) by the bar. (sof Fe = 0.444 J/(g.°C).)
3.) An iron bar with a mass of 869 g cools from 94.0 °C to 5.0 °C. Calculate the heat released (in kilojoules) by the bar. (sof Fe = 0.444 J/(g.°C).)
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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![### Thermodynamics Homework Question
**Problem Statement:**
3. An iron bar with a mass of 869 g cools from 94.0°C to 5.0°C. Calculate the heat released (in kilojoules) by the bar. (Specific heat capacity of iron, \( c_{\text{Fe}} = 0.444 \, \text{J/g°C} \)).
**Solution Explanation:**
To calculate the heat released by the iron bar as it cools, use the formula:
\[ q = mc\Delta T \]
Where:
- \( q \) is the heat transferred (in joules),
- \( m \) is the mass (in grams),
- \( c \) is the specific heat capacity (in J/g°C),
- \( \Delta T \) is the change in temperature (in °C).
**Steps for Calculation:**
1. **Determine the change in temperature (\( \Delta T \)):**
\[
\Delta T = T_{\text{final}} - T_{\text{initial}} = 5.0°C - 94.0°C = -89.0°C
\]
2. **Calculate the heat released (\( q \)):**
\[
q = mc\Delta T = (869 \, \text{g})(0.444 \, \text{J/g°C})(-89.0 \, °C)
\]
3. **Convert joules to kilojoules:**
Calculate \( q \) and then convert the result from joules to kilojoules by dividing by 1000.
The calculation will reveal the total heat energy released as the iron bar cools down to the final temperature. This process is essential to understanding thermal energy transfer in thermodynamic systems.
(No graphs or diagrams are present in the image for further explanation.)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1aa2dc25-6602-4f43-83e9-bc95506c94d5%2F38afad9d-5fbc-474e-9740-2def5ca6b093%2Fffa9bru_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Thermodynamics Homework Question
**Problem Statement:**
3. An iron bar with a mass of 869 g cools from 94.0°C to 5.0°C. Calculate the heat released (in kilojoules) by the bar. (Specific heat capacity of iron, \( c_{\text{Fe}} = 0.444 \, \text{J/g°C} \)).
**Solution Explanation:**
To calculate the heat released by the iron bar as it cools, use the formula:
\[ q = mc\Delta T \]
Where:
- \( q \) is the heat transferred (in joules),
- \( m \) is the mass (in grams),
- \( c \) is the specific heat capacity (in J/g°C),
- \( \Delta T \) is the change in temperature (in °C).
**Steps for Calculation:**
1. **Determine the change in temperature (\( \Delta T \)):**
\[
\Delta T = T_{\text{final}} - T_{\text{initial}} = 5.0°C - 94.0°C = -89.0°C
\]
2. **Calculate the heat released (\( q \)):**
\[
q = mc\Delta T = (869 \, \text{g})(0.444 \, \text{J/g°C})(-89.0 \, °C)
\]
3. **Convert joules to kilojoules:**
Calculate \( q \) and then convert the result from joules to kilojoules by dividing by 1000.
The calculation will reveal the total heat energy released as the iron bar cools down to the final temperature. This process is essential to understanding thermal energy transfer in thermodynamic systems.
(No graphs or diagrams are present in the image for further explanation.)
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