en Calculate the enthalpy change for the reaction below. + CO2(g) + (graphite) 4HNO3(1) 4NO2(g) ΔΗ (kJ/mol) -174.1 -393.5 33.2 а. -123.9 kJ b. - 472.1 kJ с. -201.9 kJ d. -404.8 kJ е. -135.9 kJ (E (A B
en Calculate the enthalpy change for the reaction below. + CO2(g) + (graphite) 4HNO3(1) 4NO2(g) ΔΗ (kJ/mol) -174.1 -393.5 33.2 а. -123.9 kJ b. - 472.1 kJ с. -201.9 kJ d. -404.8 kJ е. -135.9 kJ (E (A B
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section: Chapter Questions
Problem 50PS: The enthalpy changes of the following reactions can be measured: C2H4(g) + 3 O2(g) 2 CO2(g) + 2...
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![### QUESTION 2
#### Objective:
Calculate the enthalpy change for the reaction below.
#### Reaction:
\[ \text{C (graphite)} + 4\text{HNO}_3(l) \rightarrow \text{CO}_2(g) + 4\text{NO}_2(g) \]
#### Enthalpy (\(\Delta H\)) Values:
- \(\Delta H\) for C (graphite): \(0 \, \text{kJ/mol}\)
- \(\Delta H\) for \(4\text{HNO}_3(l)\): \(-174.1 \, \text{kJ/mol}\)
- \(\Delta H\) for \(\text{CO}_2(g)\): \(-393.5 \, \text{kJ/mol}\)
- \(\Delta H\) for \(4\text{NO}_2(g)\): \(33.2 \, \text{kJ/mol}\)
#### Options:
a. \(-123.9 \, \text{kJ}\)
b. \(-472.1 \, \text{kJ}\)
c. \(-201.9 \, \text{kJ}\)
d. \(-404.8 \, \text{kJ}\)
e. \(-135.9 \, \text{kJ}\)
#### Answer Choices:
- E
- A
- B
- D
- C
---
To calculate the enthalpy change (\(\Delta H\)) for the reaction, we use the formula:
\[ \Delta H_{\text{reaction}} = \sum \Delta H_{\text{products}} - \sum \Delta H_{\text{reactants}} \]
Substitute the given values to find the correct option.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F17050110-9897-4bd6-b477-110f723d877a%2Fd2798dea-7cbb-4ddb-b4d5-3ae27335d53d%2Fpof5cb3_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### QUESTION 2
#### Objective:
Calculate the enthalpy change for the reaction below.
#### Reaction:
\[ \text{C (graphite)} + 4\text{HNO}_3(l) \rightarrow \text{CO}_2(g) + 4\text{NO}_2(g) \]
#### Enthalpy (\(\Delta H\)) Values:
- \(\Delta H\) for C (graphite): \(0 \, \text{kJ/mol}\)
- \(\Delta H\) for \(4\text{HNO}_3(l)\): \(-174.1 \, \text{kJ/mol}\)
- \(\Delta H\) for \(\text{CO}_2(g)\): \(-393.5 \, \text{kJ/mol}\)
- \(\Delta H\) for \(4\text{NO}_2(g)\): \(33.2 \, \text{kJ/mol}\)
#### Options:
a. \(-123.9 \, \text{kJ}\)
b. \(-472.1 \, \text{kJ}\)
c. \(-201.9 \, \text{kJ}\)
d. \(-404.8 \, \text{kJ}\)
e. \(-135.9 \, \text{kJ}\)
#### Answer Choices:
- E
- A
- B
- D
- C
---
To calculate the enthalpy change (\(\Delta H\)) for the reaction, we use the formula:
\[ \Delta H_{\text{reaction}} = \sum \Delta H_{\text{products}} - \sum \Delta H_{\text{reactants}} \]
Substitute the given values to find the correct option.
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