For each reaction, find the value of ASº. Report the value with the appropriate sign. (a) 3 NO2(g) + H,O(1) → 2 HNO3(1) +NO(g) J/K (b) N2(g) + 3 F2(g) 2 NF3(g) J/K (c) C,H1,06(s) + 6 O2(g) 6 CO2(g) + 6 H,0(g) J/K
For each reaction, find the value of ASº. Report the value with the appropriate sign. (a) 3 NO2(g) + H,O(1) → 2 HNO3(1) +NO(g) J/K (b) N2(g) + 3 F2(g) 2 NF3(g) J/K (c) C,H1,06(s) + 6 O2(g) 6 CO2(g) + 6 H,0(g) J/K
Chemistry
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Chapter1: Chemical Foundations
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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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![### Calculating the Standard Entropy Change (ΔS°) for Chemical Reactions
To understand the spontaneity and feasibility of chemical reactions, it is important to calculate the standard entropy change (ΔS°). Entropy is a measure of disorder or randomness in a system. For each reaction below, you'll find the entropy change values (ΔS°) reported with the appropriate sign.
#### Reaction (a):
\[
3 \text{NO}_2(g) + \text{H}_2\text{O}(l) \rightarrow 2 \text{HNO}_3(l) + \text{NO}(g)
\]
**ΔS° Calculation:**
\[ \boxed{\text{J/K}} \]
#### Reaction (b):
\[
\text{N}_2(g) + 3 \text{F}_2(g) \rightarrow 2 \text{NF}_3(g)
\]
**ΔS° Calculation:**
\[ \boxed{\text{J/K}} \]
#### Reaction (c):
\[
\text{C}_6\text{H}_12\text{O}_6(s) + 6 \text{O}_2(g) \rightarrow 6 \text{CO}_2(g) + 6 \text{H}_2\text{O}(g)
\]
**ΔS° Calculation:**
\[ \boxed{\text{J/K}} \]
Make sure to perform the calculations based on the standard entropy values for each reactant and product involved in the reactions. The entropy change for a reaction can be calculated using the standard entropy values (S°) as follows:
\[
\Delta S° = \sum S°(\text{products}) - \sum S°(\text{reactants})
\]
In the space provided above (denoted by boxed regions), you would typically enter your computed value in Joules per Kelvin (J/K).
### Understanding the Context:
**Graphs or Diagrams**: In this particular assignment, there are no graphs or diagrams present.
Calculating the ΔS° for each reaction is a crucial step in thermodynamics as it helps in predicting whether a process will occur spontaneously. Positive values for ΔS° typically indicate increased disorder (favorable conditions) while negative values indicate decreased disorder.
Feel free to proceed with the calculations using the standard entropy values available in thermodynamic tables.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe0ae19d5-3750-41df-884f-8ca3aa31e002%2F04a804a7-d7b4-4319-95fd-ce045d6af3ed%2Fybsqi7_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Calculating the Standard Entropy Change (ΔS°) for Chemical Reactions
To understand the spontaneity and feasibility of chemical reactions, it is important to calculate the standard entropy change (ΔS°). Entropy is a measure of disorder or randomness in a system. For each reaction below, you'll find the entropy change values (ΔS°) reported with the appropriate sign.
#### Reaction (a):
\[
3 \text{NO}_2(g) + \text{H}_2\text{O}(l) \rightarrow 2 \text{HNO}_3(l) + \text{NO}(g)
\]
**ΔS° Calculation:**
\[ \boxed{\text{J/K}} \]
#### Reaction (b):
\[
\text{N}_2(g) + 3 \text{F}_2(g) \rightarrow 2 \text{NF}_3(g)
\]
**ΔS° Calculation:**
\[ \boxed{\text{J/K}} \]
#### Reaction (c):
\[
\text{C}_6\text{H}_12\text{O}_6(s) + 6 \text{O}_2(g) \rightarrow 6 \text{CO}_2(g) + 6 \text{H}_2\text{O}(g)
\]
**ΔS° Calculation:**
\[ \boxed{\text{J/K}} \]
Make sure to perform the calculations based on the standard entropy values for each reactant and product involved in the reactions. The entropy change for a reaction can be calculated using the standard entropy values (S°) as follows:
\[
\Delta S° = \sum S°(\text{products}) - \sum S°(\text{reactants})
\]
In the space provided above (denoted by boxed regions), you would typically enter your computed value in Joules per Kelvin (J/K).
### Understanding the Context:
**Graphs or Diagrams**: In this particular assignment, there are no graphs or diagrams present.
Calculating the ΔS° for each reaction is a crucial step in thermodynamics as it helps in predicting whether a process will occur spontaneously. Positive values for ΔS° typically indicate increased disorder (favorable conditions) while negative values indicate decreased disorder.
Feel free to proceed with the calculations using the standard entropy values available in thermodynamic tables.
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