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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![**Specific Heat Capacity Exercises**
1. **Problem 1: Heating Copper**
A layer of copper welded to the bottom of a skillet weighs 125 g. How much heat is needed to raise the temperature of the copper layer from 25°C to 300°C? The specific heat capacity (C) of Cu is 0.387 J/g·°C.
Calculations:
\[
q = 0.387 \frac{J}{g· K} \times 125 \text{ g} \times (300 - 25) °C = 1.33 \times 10^4 \text{ J}
\]
2. **Problem 2: Cooling Ethylene Glycol**
Find the heat transferred when 6105 g of ethylene glycol (C = 2.42 J/g·°C) when a car radiator cools from 37.0°C to 25.0°C.
3. **Problem 3: Specific Heat of Diamonds**
In a purity check for industrial diamonds, a 10.25 – carat (1 carat = 0.2000 g) diamond is heated to 74.21°C and immersed in 26.03 g of water in a constant-pressure calorimeter. The initial temperature of the water is 27.20°C. The final temperature of the system is 27.65°C. Calculate the specific heat of the diamond.
4. **Problem 4: Cooling Ethylene Glycol Sample**
A 27.7 g sample of ethylene glycol loses 688 J of heat. What was the initial temperature of the ethylene glycol if the final temperature is 32.5°C? (C of ethylene glycol = 2.42 J/g·°C).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7c430cc2-4097-4d45-9871-f052d1dcc428%2Ff414fd32-729b-4a3b-b8b0-f54ffdbac1f1%2Fajzhvj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Specific Heat Capacity Exercises**
1. **Problem 1: Heating Copper**
A layer of copper welded to the bottom of a skillet weighs 125 g. How much heat is needed to raise the temperature of the copper layer from 25°C to 300°C? The specific heat capacity (C) of Cu is 0.387 J/g·°C.
Calculations:
\[
q = 0.387 \frac{J}{g· K} \times 125 \text{ g} \times (300 - 25) °C = 1.33 \times 10^4 \text{ J}
\]
2. **Problem 2: Cooling Ethylene Glycol**
Find the heat transferred when 6105 g of ethylene glycol (C = 2.42 J/g·°C) when a car radiator cools from 37.0°C to 25.0°C.
3. **Problem 3: Specific Heat of Diamonds**
In a purity check for industrial diamonds, a 10.25 – carat (1 carat = 0.2000 g) diamond is heated to 74.21°C and immersed in 26.03 g of water in a constant-pressure calorimeter. The initial temperature of the water is 27.20°C. The final temperature of the system is 27.65°C. Calculate the specific heat of the diamond.
4. **Problem 4: Cooling Ethylene Glycol Sample**
A 27.7 g sample of ethylene glycol loses 688 J of heat. What was the initial temperature of the ethylene glycol if the final temperature is 32.5°C? (C of ethylene glycol = 2.42 J/g·°C).
![### Worksheet: Heat of Reaction
#### Instructions:
Use the given standard enthalpies of formation to determine the heat of reaction of the following reactions:
### Note: Heat of formation of elements is 0.
#### Enthalpy Data (ΔH⁰f):
- **N₂H₄(l)**: +50.6 kJ/mole
- **H₂O(l)**: -285.9 kJ/mole
- **CO₂(g)**: -393.5 kJ/mole
- **C₆H₁₂(l)**: -156.4 kJ/mole
- **C₅H₁₂O(l)**: -249.5 kJ/mole
- **CS₂(l)**: +117.4 kJ/mole
- **SO₂(g)**: -296.8 kJ/mole
### Problems:
**1. Calculate the heat of reaction for:**
\[ \text{N}_2\text{H}_4(l) + O_2(g) \rightarrow \text{N}_2(g) + 2\text{H}_2\text{O}(l) \]
**2. Calculate the heat of reaction for:**
\[ \text{C}_5\text{H}_{12}\text{O}(l) + 4O_2(g) \rightarrow 5CO_2(g) + 3H_2O(l) \]
**3. Calculate the heat of reaction for:**
\[ \text{CS}_2(l) + 3O_2(g) \rightarrow CO_2(g) + 2SO_2(g) \]
**4. The combustion of cyclohexane C₆H₁₂.**
\[ C_6H_{12(l)} + 9O_2(g) \rightarrow 6CO_2(g) + 6H_2O(l) \]
### Solution Guidelines:
1. **For each reaction:**
- Use the provided enthalpy values and the formula:
\[
\Delta H = \sum(\Delta H_{\text{products}}) - \sum(\Delta H_{\text{reactants}})
\]
- Apply stoichiometry to ensure each compound's molar quantities are accounted for.
### Example Calculation:
For reaction 1: \[ \text{N}_2\](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7c430cc2-4097-4d45-9871-f052d1dcc428%2Ff414fd32-729b-4a3b-b8b0-f54ffdbac1f1%2Fhlrjx6_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Worksheet: Heat of Reaction
#### Instructions:
Use the given standard enthalpies of formation to determine the heat of reaction of the following reactions:
### Note: Heat of formation of elements is 0.
#### Enthalpy Data (ΔH⁰f):
- **N₂H₄(l)**: +50.6 kJ/mole
- **H₂O(l)**: -285.9 kJ/mole
- **CO₂(g)**: -393.5 kJ/mole
- **C₆H₁₂(l)**: -156.4 kJ/mole
- **C₅H₁₂O(l)**: -249.5 kJ/mole
- **CS₂(l)**: +117.4 kJ/mole
- **SO₂(g)**: -296.8 kJ/mole
### Problems:
**1. Calculate the heat of reaction for:**
\[ \text{N}_2\text{H}_4(l) + O_2(g) \rightarrow \text{N}_2(g) + 2\text{H}_2\text{O}(l) \]
**2. Calculate the heat of reaction for:**
\[ \text{C}_5\text{H}_{12}\text{O}(l) + 4O_2(g) \rightarrow 5CO_2(g) + 3H_2O(l) \]
**3. Calculate the heat of reaction for:**
\[ \text{CS}_2(l) + 3O_2(g) \rightarrow CO_2(g) + 2SO_2(g) \]
**4. The combustion of cyclohexane C₆H₁₂.**
\[ C_6H_{12(l)} + 9O_2(g) \rightarrow 6CO_2(g) + 6H_2O(l) \]
### Solution Guidelines:
1. **For each reaction:**
- Use the provided enthalpy values and the formula:
\[
\Delta H = \sum(\Delta H_{\text{products}}) - \sum(\Delta H_{\text{reactants}})
\]
- Apply stoichiometry to ensure each compound's molar quantities are accounted for.
### Example Calculation:
For reaction 1: \[ \text{N}_2\
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