WA d. If 2500. kJ of heat are released by the reaction, how grams of Ciz been consumed/used? or world with shor ont ran Show of a hipq ni swaro vinebbus tous e. If this reaction were being used to generate heat, how many gra would have to be reacted to generate enough heat to raise the 250g of liquid water from 10°C to 85°C (remember that the Cp of 4.184J/g°C, and find the energy needed for this change first.)
WA d. If 2500. kJ of heat are released by the reaction, how grams of Ciz been consumed/used? or world with shor ont ran Show of a hipq ni swaro vinebbus tous e. If this reaction were being used to generate heat, how many gra would have to be reacted to generate enough heat to raise the 250g of liquid water from 10°C to 85°C (remember that the Cp of 4.184J/g°C, and find the energy needed for this change first.)
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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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
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Please help with 2 d-e
![**Thermochemistry and Reaction Calculations**
**Problem 2: Analyzing a Thermochemical Reaction**
Consider the following thermochemical reaction for kerosene:
\[ 2 \; \text{C}_{12}\text{H}_{26}(l) + 37 \; \text{O}_2(g) \rightarrow 24 \; \text{CO}_2(g) + 26 \; \text{H}_2\text{O}(l) \]
\[ \Delta H = -15,026 \; \text{kJ} \]
**Tasks:**
a. **Write Equivalence Statements**
- Using the enthalpy of the reaction, equivalence statements should be written to relate energy to mole amounts of reactants and products.
b. **Energy Level Diagram**
- Illustrate an energy level diagram for this process. The diagram should show the relative energy levels of reactants and products, with arrows indicating the energy change (ΔH).
c. **Calculation for CO₂ Formation**
- Determine the amount of heat released when 43.2 g of CO₂ are produced. Express energy as an equivalent statement in terms of moles. (Use known molar mass values for calculations.)
d. **Calculating Kerosene Consumption**
- Given that 2500 kJ of heat are released, calculate how many grams of C₁₂H₂₆ must have been consumed/used in the reaction.
e. **Heat Exchange and Reaction Use**
- Calculate how many grams of C₁₂H₂₆ must be reacted to generate enough heat to raise the temperature of 250 g of water from 10°C to 85°C. Consider the specific heat capacity (Cp) of water to be 4.184 J/g°C, and compute the required energy for this temperature change first.
**Diagram Explanation:**
- The diagram appears to have a downward slope starting at the energy level of the reactants and ending at the lower energy level of the products. This indicates an exothermic reaction with a decrease in enthalpy, depicted by the negative ΔH value.
These steps provide insights into thermochemical processes and equip learners with the ability to carry out energy-related calculations involving chemical reactions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa7e1480f-493b-4334-b48e-1a7032a37693%2F7626d6d7-52b1-4971-a0ed-99833d925c32%2Fcsz2il_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Thermochemistry and Reaction Calculations**
**Problem 2: Analyzing a Thermochemical Reaction**
Consider the following thermochemical reaction for kerosene:
\[ 2 \; \text{C}_{12}\text{H}_{26}(l) + 37 \; \text{O}_2(g) \rightarrow 24 \; \text{CO}_2(g) + 26 \; \text{H}_2\text{O}(l) \]
\[ \Delta H = -15,026 \; \text{kJ} \]
**Tasks:**
a. **Write Equivalence Statements**
- Using the enthalpy of the reaction, equivalence statements should be written to relate energy to mole amounts of reactants and products.
b. **Energy Level Diagram**
- Illustrate an energy level diagram for this process. The diagram should show the relative energy levels of reactants and products, with arrows indicating the energy change (ΔH).
c. **Calculation for CO₂ Formation**
- Determine the amount of heat released when 43.2 g of CO₂ are produced. Express energy as an equivalent statement in terms of moles. (Use known molar mass values for calculations.)
d. **Calculating Kerosene Consumption**
- Given that 2500 kJ of heat are released, calculate how many grams of C₁₂H₂₆ must have been consumed/used in the reaction.
e. **Heat Exchange and Reaction Use**
- Calculate how many grams of C₁₂H₂₆ must be reacted to generate enough heat to raise the temperature of 250 g of water from 10°C to 85°C. Consider the specific heat capacity (Cp) of water to be 4.184 J/g°C, and compute the required energy for this temperature change first.
**Diagram Explanation:**
- The diagram appears to have a downward slope starting at the energy level of the reactants and ending at the lower energy level of the products. This indicates an exothermic reaction with a decrease in enthalpy, depicted by the negative ΔH value.
These steps provide insights into thermochemical processes and equip learners with the ability to carry out energy-related calculations involving chemical reactions.
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