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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I need help on #14
![### Educational Website Content: Thermodynamics Quiz Questions
---
**14) How much heat is needed to raise the temperature of 25 grams of water at 20°C to 85°C?**
a) 3283J
b) 3348J
c) 4865J
d) 6793J
---
**15) How much heat is released when 17 grams of water at 45°C changes to ice at -20°C?**
a) -5678 J
b) -3197.7 J
c) -9576.1 J
d) -25,458 J
---
**Explanation:**
1. **Question 14: Calculation of Heat**
- To determine the amount of heat (Q) needed to raise the temperature, use the formula:
\[ Q = m \cdot c \cdot \Delta T \]
Where:
- \( m \) = mass of the water (25 grams)
- \( c \) = specific heat capacity of water (\( 4.18\ J/g^\circ C \))
- \( \Delta T \) = change in temperature (\( 85^\circ C - 20^\circ C \))
- Substitute values to find the answer.
2. **Question 15: Heat Released During Phase Change**
- The calculation involves two steps: cooling water from 45°C to 0°C, and then the phase change from water to ice, and finally cooling the ice to -20°C.
- Cooling water: Use the formula \( Q = m \cdot c \cdot \Delta T \).
- Phase change: Use the latent heat of fusion for water (\( 334\ J/g \)).
- Cooling ice: Use the specific heat capacity of ice (\( 2.09\ J/g^\circ C \)).
- Add the heat changes to get the total heat released.
This section deals with practical applications of thermodynamic principles in calculating heat transfer during changes in temperature and phase of water. To practice these calculations, ensure understanding of concepts such as specific heat capacity, latent heat, and the respective formulas.
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Transcribed Image Text:### Educational Website Content: Thermodynamics Quiz Questions
---
**14) How much heat is needed to raise the temperature of 25 grams of water at 20°C to 85°C?**
a) 3283J
b) 3348J
c) 4865J
d) 6793J
---
**15) How much heat is released when 17 grams of water at 45°C changes to ice at -20°C?**
a) -5678 J
b) -3197.7 J
c) -9576.1 J
d) -25,458 J
---
**Explanation:**
1. **Question 14: Calculation of Heat**
- To determine the amount of heat (Q) needed to raise the temperature, use the formula:
\[ Q = m \cdot c \cdot \Delta T \]
Where:
- \( m \) = mass of the water (25 grams)
- \( c \) = specific heat capacity of water (\( 4.18\ J/g^\circ C \))
- \( \Delta T \) = change in temperature (\( 85^\circ C - 20^\circ C \))
- Substitute values to find the answer.
2. **Question 15: Heat Released During Phase Change**
- The calculation involves two steps: cooling water from 45°C to 0°C, and then the phase change from water to ice, and finally cooling the ice to -20°C.
- Cooling water: Use the formula \( Q = m \cdot c \cdot \Delta T \).
- Phase change: Use the latent heat of fusion for water (\( 334\ J/g \)).
- Cooling ice: Use the specific heat capacity of ice (\( 2.09\ J/g^\circ C \)).
- Add the heat changes to get the total heat released.
This section deals with practical applications of thermodynamic principles in calculating heat transfer during changes in temperature and phase of water. To practice these calculations, ensure understanding of concepts such as specific heat capacity, latent heat, and the respective formulas.
---
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