Nitrogen monoxide has been found to react with oxygen gas to produce the brown gas nitrogen dioxide. When one mole of no reacts with oxygen, 57.0 kJ of heat is released. a. Write the thermochemical equation for the reaction between one mole of nitrogen monoxide and oxygen to produce nitrogen dioxide. b. Is the reaction exothermic or endothermic? c. What is AH when 5.00 g of nitrogen monoxide reacts? d. How many grams of nitrogen monoxide must react with an excess of oxygen to produce 10.0 kJ of heat?
Nitrogen monoxide has been found to react with oxygen gas to produce the brown gas nitrogen dioxide. When one mole of no reacts with oxygen, 57.0 kJ of heat is released. a. Write the thermochemical equation for the reaction between one mole of nitrogen monoxide and oxygen to produce nitrogen dioxide. b. Is the reaction exothermic or endothermic? c. What is AH when 5.00 g of nitrogen monoxide reacts? d. How many grams of nitrogen monoxide must react with an excess of oxygen to produce 10.0 kJ of heat?
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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Hi sorry to bother I know that you guys can only answer 3 questions per the ask questions so I was wondering if you could solve the following 3 for me please thank you
![**Thermochemical Reactions: Understanding Nitrogen Monoxide and Oxygen Reactions**
In this exercise, we will explore the reaction of nitrogen monoxide with oxygen to produce nitrogen dioxide. As you follow along, consider the following questions and concepts to deepen your understanding of thermochemical reactions.
**Problem Statement:**
4. Nitrogen monoxide has been found to react with oxygen gas to produce the brown gas nitrogen dioxide. When one mole of nitrogen monoxide reacts with oxygen, 57.0 kJ of heat is released.
a. Write the thermochemical equation for the reaction between one mole of nitrogen monoxide and oxygen to produce nitrogen dioxide.
b. Is the reaction exothermic or endothermic?
c. What is ΔH when 5.00 g of nitrogen monoxide reacts?
d. How many grams of nitrogen monoxide must react with an excess of oxygen to produce 10.0 kJ of heat?
**Explaining Key Concepts with Graphs and Diagrams:**
1. **Thermochemical Equation:**
When nitrogen monoxide (NO) reacts with oxygen (O₂) to produce nitrogen dioxide (NO₂), the thermochemical equation can be written to include the heat change (ΔH):
\[
2NO (g) + O₂ (g) \rightarrow 2NO₂ (g) \quad \Delta H = -114 \text{ kJ}
\]
This indicates that the reaction releases 114 kJ of heat for 2 moles of NO reacting, hence -57 kJ for one mole.
2. **Exothermic vs. Endothermic Reactions:**
- An **exothermic reaction** releases heat to the surroundings, causing the temperature of the surroundings to increase.
- An **endothermic reaction** absorbs heat from the surroundings, causing the temperature of the surroundings to decrease.
Since 57.0 kJ of heat is released, this reaction is exothermic.
3. **Calculating ΔH for a Given Mass:**
To find ΔH for 5.00 g of NO reacting, convert the mass to moles and use the ΔH per mole of NO:
- Molar mass of NO = 14 (N) + 16 (O) = 30 g/mol
- Moles of NO = \( \frac{5.00 \text{ g}}{30 \text{ g/mol}} = 0.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7c430cc2-4097-4d45-9871-f052d1dcc428%2F5a6d7e07-16ad-4abe-a061-e61dca682d36%2Fvpveby8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Thermochemical Reactions: Understanding Nitrogen Monoxide and Oxygen Reactions**
In this exercise, we will explore the reaction of nitrogen monoxide with oxygen to produce nitrogen dioxide. As you follow along, consider the following questions and concepts to deepen your understanding of thermochemical reactions.
**Problem Statement:**
4. Nitrogen monoxide has been found to react with oxygen gas to produce the brown gas nitrogen dioxide. When one mole of nitrogen monoxide reacts with oxygen, 57.0 kJ of heat is released.
a. Write the thermochemical equation for the reaction between one mole of nitrogen monoxide and oxygen to produce nitrogen dioxide.
b. Is the reaction exothermic or endothermic?
c. What is ΔH when 5.00 g of nitrogen monoxide reacts?
d. How many grams of nitrogen monoxide must react with an excess of oxygen to produce 10.0 kJ of heat?
**Explaining Key Concepts with Graphs and Diagrams:**
1. **Thermochemical Equation:**
When nitrogen monoxide (NO) reacts with oxygen (O₂) to produce nitrogen dioxide (NO₂), the thermochemical equation can be written to include the heat change (ΔH):
\[
2NO (g) + O₂ (g) \rightarrow 2NO₂ (g) \quad \Delta H = -114 \text{ kJ}
\]
This indicates that the reaction releases 114 kJ of heat for 2 moles of NO reacting, hence -57 kJ for one mole.
2. **Exothermic vs. Endothermic Reactions:**
- An **exothermic reaction** releases heat to the surroundings, causing the temperature of the surroundings to increase.
- An **endothermic reaction** absorbs heat from the surroundings, causing the temperature of the surroundings to decrease.
Since 57.0 kJ of heat is released, this reaction is exothermic.
3. **Calculating ΔH for a Given Mass:**
To find ΔH for 5.00 g of NO reacting, convert the mass to moles and use the ΔH per mole of NO:
- Molar mass of NO = 14 (N) + 16 (O) = 30 g/mol
- Moles of NO = \( \frac{5.00 \text{ g}}{30 \text{ g/mol}} = 0.
![**Thermochemical Reactions: Strontium and Cupric Oxide**
**5. Strontium Metal Combines with Graphite and Oxygen Gas:**
Strontium metal can combine with graphite (C) and oxygen gas (O2) to produce strontium carbonate (SrCO3). The formation of one mole of SrCO3 releases 1,220 kJ of heat.
a. **Balanced Thermochemical Equation:**
Write a balanced thermochemical equation for the reaction resulting in one mole of SrCO3.
b. **Calculation of ΔH:**
What is ΔH when 100.0 g of strontium reacts with excess graphite and oxygen?
c. **Mass Formation:**
What mass of SrCO3 forms when 2,355 kJ of heat are also formed?
**6. Reaction of Cupric Oxide and Determination of Heat of Formation:**
Given the reaction:
\[ 2CuO(s) \rightarrow 2Cu(s) + O_2(g) \quad \Delta H = 314.6 \text{kJ} \]
a. **Heat of Formation:**
Determine the heat of formation of CuO(s).
b. **Calculation of ΔH:**
Calculate ΔH for the formation of 13.58 g of CuO.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7c430cc2-4097-4d45-9871-f052d1dcc428%2F5a6d7e07-16ad-4abe-a061-e61dca682d36%2Fa63v68b_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Thermochemical Reactions: Strontium and Cupric Oxide**
**5. Strontium Metal Combines with Graphite and Oxygen Gas:**
Strontium metal can combine with graphite (C) and oxygen gas (O2) to produce strontium carbonate (SrCO3). The formation of one mole of SrCO3 releases 1,220 kJ of heat.
a. **Balanced Thermochemical Equation:**
Write a balanced thermochemical equation for the reaction resulting in one mole of SrCO3.
b. **Calculation of ΔH:**
What is ΔH when 100.0 g of strontium reacts with excess graphite and oxygen?
c. **Mass Formation:**
What mass of SrCO3 forms when 2,355 kJ of heat are also formed?
**6. Reaction of Cupric Oxide and Determination of Heat of Formation:**
Given the reaction:
\[ 2CuO(s) \rightarrow 2Cu(s) + O_2(g) \quad \Delta H = 314.6 \text{kJ} \]
a. **Heat of Formation:**
Determine the heat of formation of CuO(s).
b. **Calculation of ΔH:**
Calculate ΔH for the formation of 13.58 g of CuO.
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