Calculate the energy required to heat 486.0 mg of silver from -9.6 °C to -3.7 °C. Assume the specific heat capacity of silver under these conditions is 0.235 J-gK . Round your answer to 2 significant digits. olo
Calculate the energy required to heat 486.0 mg of silver from -9.6 °C to -3.7 °C. Assume the specific heat capacity of silver under these conditions is 0.235 J-gK . Round your answer to 2 significant digits. olo
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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Thermodynamics: Using Specific Heat Capacity to Find Heat**
Calculate the energy required to heat 486.0 mg of silver from -9.6 °C to -3.7 °C. Assume the specific heat capacity of silver under these conditions is 0.235 J·g⁻¹·K⁻¹. Round your answer to 2 significant digits.
**Explanation:**
To solve this problem, you can use the formula for calculating heat energy (q):
\[ q = m \cdot c \cdot \Delta T \]
Where:
- \( q \) is the heat energy in joules (J).
- \( m \) is the mass of the substance in grams (g).
- \( c \) is the specific heat capacity in J·g⁻¹·K⁻¹.
- \( \Delta T \) is the change in temperature in degrees Celsius (°C) or Kelvin (K).
1. **Convert the mass of silver from mg to g:**
- 486.0 mg = 0.4860 g
2. **Calculate the change in temperature (\( \Delta T \)):**
- \( \Delta T = (-3.7 °C) - (-9.6 °C) = 5.9 °C \)
3. **Plug the values into the formula:**
- \( q = 0.4860 \text{ g} \times 0.235 \text{ J·g⁻}¹·\text{K⁻}¹ \times 5.9 \text{ K} \)
4. **Calculate \( q \):**
- \( q \approx 0.67224 \text{ J} \)
5. **Round the answer to 2 significant digits:**
- \( q \approx 0.67 \text{ J} \)
**Graph/Diagram Explanation:**
There are no graphs or diagrams included in this image.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffa5d4b72-0f64-47a2-aa28-ebb729836a09%2Fc8740c4f-6368-425e-b97b-d0de0ff84278%2F4vp57v_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Thermodynamics: Using Specific Heat Capacity to Find Heat**
Calculate the energy required to heat 486.0 mg of silver from -9.6 °C to -3.7 °C. Assume the specific heat capacity of silver under these conditions is 0.235 J·g⁻¹·K⁻¹. Round your answer to 2 significant digits.
**Explanation:**
To solve this problem, you can use the formula for calculating heat energy (q):
\[ q = m \cdot c \cdot \Delta T \]
Where:
- \( q \) is the heat energy in joules (J).
- \( m \) is the mass of the substance in grams (g).
- \( c \) is the specific heat capacity in J·g⁻¹·K⁻¹.
- \( \Delta T \) is the change in temperature in degrees Celsius (°C) or Kelvin (K).
1. **Convert the mass of silver from mg to g:**
- 486.0 mg = 0.4860 g
2. **Calculate the change in temperature (\( \Delta T \)):**
- \( \Delta T = (-3.7 °C) - (-9.6 °C) = 5.9 °C \)
3. **Plug the values into the formula:**
- \( q = 0.4860 \text{ g} \times 0.235 \text{ J·g⁻}¹·\text{K⁻}¹ \times 5.9 \text{ K} \)
4. **Calculate \( q \):**
- \( q \approx 0.67224 \text{ J} \)
5. **Round the answer to 2 significant digits:**
- \( q \approx 0.67 \text{ J} \)
**Graph/Diagram Explanation:**
There are no graphs or diagrams included in this image.
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