Hasis fint 526 ms! 2. Consider the following thermochemical reaction for kerosene: 2 C12H26 (1) +37 O2(g) → 24 CO2(g) + 26 H₂O(1) AH = -15,026 kJ a. Write all 4 equivalence statements using the enthalpy of the reaction. (energy to mole amounts) C. bilea b. Show an energy level diagram for this process. ontwolofanl When 43.2 g of CO2 are made, how much heat is released? (hint, write the energy as an equivalent statement with moles like was shown in class) polled tornion 600 pn llam lerme d. If 2500. kJ of heat are released by the reaction, how grams of C12H26 must have been consumed/used? 1101 e. If this reaction were being used to generate heat, how many grams of C12H26 would have to be reacted to generate enough heat to raise the temperature of 250g of liquid water from 10°C to 85°C (remember that the Cp of water is 4.184J/g°C, and find the energy needed for this change first.)
Hasis fint 526 ms! 2. Consider the following thermochemical reaction for kerosene: 2 C12H26 (1) +37 O2(g) → 24 CO2(g) + 26 H₂O(1) AH = -15,026 kJ a. Write all 4 equivalence statements using the enthalpy of the reaction. (energy to mole amounts) C. bilea b. Show an energy level diagram for this process. ontwolofanl When 43.2 g of CO2 are made, how much heat is released? (hint, write the energy as an equivalent statement with moles like was shown in class) polled tornion 600 pn llam lerme d. If 2500. kJ of heat are released by the reaction, how grams of C12H26 must have been consumed/used? 1101 e. If this reaction were being used to generate heat, how many grams of C12H26 would have to be reacted to generate enough heat to raise the temperature of 250g of liquid water from 10°C to 85°C (remember that the Cp of water is 4.184J/g°C, and find the energy needed for this change first.)
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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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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6c605e87-2c96-4aa2-99a1-2c5d12ea3556%2Ffbc27c06-ce60-45dd-be65-ec5461225c80%2Fyjcp8wn_processed.jpeg&w=3840&q=75)
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
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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