ORE HEAT PRACTICE The data below refers to an unknown substance, X. Melting point Boiling Heat of Heat of Point Fusion Vaporization 695 kJ/g 425 kJ/g 1. Draw a heating curve for substance X, going from 32.0°C 112.0°C 125 Call formulas used to calculate heat. 112°C 32 °C- E gomblik! F Em SS AT SH SH Capacity (solid) (liquid) 2.3 J/gºC 5.9 J/gºC 1.1 J/gºC 15°C to 125°C on the axis below. Write in A GEMSVAT C. qm Hvap e. Find the final temperature if 150g of X, at q=ms, AT 15°C- b. Determine the amount of heat released when 15.0g of gaseous X at 112.0°C changes to liquid at 112.0°C. 9-10425K) 9=15.09x695k/g q=mal vaporization AH = 695k/g c. Determine the amount of heat necessary to convert 15.0g of solid X at-32.0°C to liquid at 32.0° C. 95 ΔΗ = d. Determine the mass of X that can be heated from-38°C to 102°C using 4500J of heat. m= AH receives 650J of heat. SH (vapor) AH-
ORE HEAT PRACTICE The data below refers to an unknown substance, X. Melting point Boiling Heat of Heat of Point Fusion Vaporization 695 kJ/g 425 kJ/g 1. Draw a heating curve for substance X, going from 32.0°C 112.0°C 125 Call formulas used to calculate heat. 112°C 32 °C- E gomblik! F Em SS AT SH SH Capacity (solid) (liquid) 2.3 J/gºC 5.9 J/gºC 1.1 J/gºC 15°C to 125°C on the axis below. Write in A GEMSVAT C. qm Hvap e. Find the final temperature if 150g of X, at q=ms, AT 15°C- b. Determine the amount of heat released when 15.0g of gaseous X at 112.0°C changes to liquid at 112.0°C. 9-10425K) 9=15.09x695k/g q=mal vaporization AH = 695k/g c. Determine the amount of heat necessary to convert 15.0g of solid X at-32.0°C to liquid at 32.0° C. 95 ΔΗ = d. Determine the mass of X that can be heated from-38°C to 102°C using 4500J of heat. m= AH receives 650J of heat. SH (vapor) AH-
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
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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Question
Answer “D”
![## Core Heat Practice
The data below refers to an unknown substance, X:
- **Melting Point:** 32.0°C
- **Boiling Point:** 112.0°C
- **Heat of Fusion:** 425 J/g
- **Heat of Vaporization:** 695 J/g
- **Specific Heat (Solid):** 2.3 J/g°C
- **Specific Heat (Liquid):** 5.9 J/g°C
- **Specific Heat (Vapor):** 1.1 J/g°C
### Instructions:
1. **Draw a heating curve for substance X,** going from 15°C to 125°C on the axis below. Include all formulas used to calculate heat.
- The diagram illustrates various segments labeled A to F:
- **A:** Represents heating of the vapor phase using the formula \( q = m \cdot s_v \cdot \Delta T \).
- **B - C:** Represents condensation using the formula \( q = m \cdot \Delta H_{vap} \).
- **C - D:** Represents heating of the liquid phase using the formula \( q = m \cdot s_l \cdot \Delta T \).
- **D - E:** Represents fusion using the formula \( q = m \cdot \Delta H_{fus} \).
- **E - F:** Represents heating of the solid phase using the formula \( q = m \cdot s_s \cdot \Delta T \).
2. **Problem Solving:**
b. **Determine the amount of heat released** when 15.0g of gaseous X at 112.0°C changes to liquid at 112.0°C.
\[
q = 15.0 \, \text{g} \times 695 \, \text{J/g} = 10425 \, \text{J}
\]
- Formula: \( q = m \cdot \Delta H_{vaporization} \)
c. **Determine the amount of heat necessary** to convert 15.0g of solid X at 32.0°C to liquid at 32.0°C.
- Fill in the formula and solution.
d. **Determine the mass of X** that can be heated from -38°C to 102°C using 4500J of heat.
-](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F277e2bd6-aa16-4b9b-8eff-85b37a6d58e3%2F5f3765dc-e8e6-4972-9d44-5e2590db6cf3%2Fknopzwq_processed.jpeg&w=3840&q=75)
Transcribed Image Text:## Core Heat Practice
The data below refers to an unknown substance, X:
- **Melting Point:** 32.0°C
- **Boiling Point:** 112.0°C
- **Heat of Fusion:** 425 J/g
- **Heat of Vaporization:** 695 J/g
- **Specific Heat (Solid):** 2.3 J/g°C
- **Specific Heat (Liquid):** 5.9 J/g°C
- **Specific Heat (Vapor):** 1.1 J/g°C
### Instructions:
1. **Draw a heating curve for substance X,** going from 15°C to 125°C on the axis below. Include all formulas used to calculate heat.
- The diagram illustrates various segments labeled A to F:
- **A:** Represents heating of the vapor phase using the formula \( q = m \cdot s_v \cdot \Delta T \).
- **B - C:** Represents condensation using the formula \( q = m \cdot \Delta H_{vap} \).
- **C - D:** Represents heating of the liquid phase using the formula \( q = m \cdot s_l \cdot \Delta T \).
- **D - E:** Represents fusion using the formula \( q = m \cdot \Delta H_{fus} \).
- **E - F:** Represents heating of the solid phase using the formula \( q = m \cdot s_s \cdot \Delta T \).
2. **Problem Solving:**
b. **Determine the amount of heat released** when 15.0g of gaseous X at 112.0°C changes to liquid at 112.0°C.
\[
q = 15.0 \, \text{g} \times 695 \, \text{J/g} = 10425 \, \text{J}
\]
- Formula: \( q = m \cdot \Delta H_{vaporization} \)
c. **Determine the amount of heat necessary** to convert 15.0g of solid X at 32.0°C to liquid at 32.0°C.
- Fill in the formula and solution.
d. **Determine the mass of X** that can be heated from -38°C to 102°C using 4500J of heat.
-
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