O THERMOCHEMISTRY Calculating specific heat capacity A chemist carefully measures the amount of heat needed to raise the temperature of a 577.0 g sample of a pure substance from 1.7 °C to 12.8 °C. The experiment shows that 890. J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits.
O THERMOCHEMISTRY Calculating specific heat capacity A chemist carefully measures the amount of heat needed to raise the temperature of a 577.0 g sample of a pure substance from 1.7 °C to 12.8 °C. The experiment shows that 890. J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits.
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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
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![**Thermochemistry: Calculating Specific Heat Capacity**
A chemist carefully measures the amount of heat needed to raise the temperature of a 577.0 g sample of a pure substance from 1.7 °C to 12.8 °C. The experiment shows that 890. J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits.
**Formula Input:**
\[ \text{J} \cdot \text{g}^{-1} \cdot \text{K}^{-1} \]
There is an input box for entering the calculated specific heat capacity value. The tools available include the ability to:
- Input scientific notation.
- Clear the entry.
- Access help or hints.
The bottom options include:
- Explanation
- Check
The task involves calculating the specific heat capacity using the formula:
\[ c = \frac{q}{m \cdot \Delta T} \]
Where:
- \( c \) is the specific heat capacity,
- \( q \) is the heat added (890. J),
- \( m \) is the mass (577.0 g),
- \( \Delta T \) is the change in temperature (12.8 °C - 1.7 °C).
**Note:** The answer should be reported with the correct number of significant digits based on the given data.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F65515c45-3543-4133-8f93-375c795a6bf2%2F393ac95a-421f-4345-952d-8cd5deeb7f9e%2Fy20rx1n_processed.png&w=3840&q=75)
Transcribed Image Text:**Thermochemistry: Calculating Specific Heat Capacity**
A chemist carefully measures the amount of heat needed to raise the temperature of a 577.0 g sample of a pure substance from 1.7 °C to 12.8 °C. The experiment shows that 890. J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits.
**Formula Input:**
\[ \text{J} \cdot \text{g}^{-1} \cdot \text{K}^{-1} \]
There is an input box for entering the calculated specific heat capacity value. The tools available include the ability to:
- Input scientific notation.
- Clear the entry.
- Access help or hints.
The bottom options include:
- Explanation
- Check
The task involves calculating the specific heat capacity using the formula:
\[ c = \frac{q}{m \cdot \Delta T} \]
Where:
- \( c \) is the specific heat capacity,
- \( q \) is the heat added (890. J),
- \( m \) is the mass (577.0 g),
- \( \Delta T \) is the change in temperature (12.8 °C - 1.7 °C).
**Note:** The answer should be reported with the correct number of significant digits based on the given data.
Expert Solution
Step 1
Given:
The mass of the substance = 577.0 g
The initial temperature of the substance = 1.7 oC
The final temperature of the substance = 12.8 oC
The amount of heat needed to raise the temperature of the substance = 890 J
We have to calculate the specific heat capacity of the substance.
Step by step
Solved in 2 steps with 1 images
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