Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Please help with question 2!
![## Thermochemical Calculations for Kerosene Combustion
### Problem 1:
**Initial Condition:**
A 10.712g block of metal receives 6.795 kJ of heat, resulting in a temperature increase of 11.4°C.
**Task:**
Calculate the specific heat capacity of the metal in J/g°C.
---
### Problem 2:
**Consideration:**
The thermochemical reaction for kerosene is given as:
\[ 2 \, \text{C}_{12}\text{H}_{26(l)} + 37 \, \text{O}_{2(g)} \rightarrow 24 \, \text{CO}_{2(g)} + 26 \, \text{H}_2\text{O}_{(l)} \]
\[ \Delta H = -15,026 \, \text{kJ} \]
#### (a) Equivalence Statements
Write four equivalence statements using the enthalpy of the reaction, focusing on energy to mole amounts.
#### (b) Energy Level Diagram
Illustrate the energy level diagram for this process.
#### (c) Heat Release Calculation
If 43.2 g of CO₂ are produced, calculate the amount of heat released. (Hint: Write the energy as an equivalent statement with moles, similar to what was shown in class.)
#### (d) Reactant Consumption
Determine how many grams of C₁₂H₂₆ are consumed if 2500 kJ of heat is released.
#### (e) Heat Generation Application
Calculate the grams of C₁₂H₂₆ needed to provide enough heat to raise the temperature of 250 g of liquid water from 10°C to 85°C. Use the specific heat capacity of water, \( \text{Cp} = 4.184 \, \text{J/g°C} \), and calculate the energy required for this temperature change first.](https://content.bartleby.com/qna-images/question/6c605e87-2c96-4aa2-99a1-2c5d12ea3556/fbc27c06-ce60-45dd-be65-ec5461225c80/yjcp8wn_processed.jpeg)
Transcribed Image Text:## Thermochemical Calculations for Kerosene Combustion
### Problem 1:
**Initial Condition:**
A 10.712g block of metal receives 6.795 kJ of heat, resulting in a temperature increase of 11.4°C.
**Task:**
Calculate the specific heat capacity of the metal in J/g°C.
---
### Problem 2:
**Consideration:**
The thermochemical reaction for kerosene is given as:
\[ 2 \, \text{C}_{12}\text{H}_{26(l)} + 37 \, \text{O}_{2(g)} \rightarrow 24 \, \text{CO}_{2(g)} + 26 \, \text{H}_2\text{O}_{(l)} \]
\[ \Delta H = -15,026 \, \text{kJ} \]
#### (a) Equivalence Statements
Write four equivalence statements using the enthalpy of the reaction, focusing on energy to mole amounts.
#### (b) Energy Level Diagram
Illustrate the energy level diagram for this process.
#### (c) Heat Release Calculation
If 43.2 g of CO₂ are produced, calculate the amount of heat released. (Hint: Write the energy as an equivalent statement with moles, similar to what was shown in class.)
#### (d) Reactant Consumption
Determine how many grams of C₁₂H₂₆ are consumed if 2500 kJ of heat is released.
#### (e) Heat Generation Application
Calculate the grams of C₁₂H₂₆ needed to provide enough heat to raise the temperature of 250 g of liquid water from 10°C to 85°C. Use the specific heat capacity of water, \( \text{Cp} = 4.184 \, \text{J/g°C} \), and calculate the energy required for this temperature change first.
Expert Solution
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Step 1
#2:
The balanced thermochemical equation for the combustion of kerosine is:
2C12H16(l) + 37O2(g) 24CO2(g) + 26H2O(l) ; H = - 15.026 kJ
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