1. The value of the standard molar entropy of N₂(g) at 298K is 191.6 J/Kmole (Table 2C.7) a. If we assume that the value of the heat capacity is independent of temperature and has the value of 29.13 J/Kmole, calculate the value of the standard molar entropy of N₂(g) at 373K. b. In reality, the molar heat capacity of N₂(g) in the range 200 K to 400 K is given by Cp,m = 28.58 +3.77x10-³T (K-¹) In which the value of Cp,m has units of J/Kmole. Using this relationship, calculate the value of the standard molar entropy of N₂(g) at 373 K.
1. The value of the standard molar entropy of N₂(g) at 298K is 191.6 J/Kmole (Table 2C.7) a. If we assume that the value of the heat capacity is independent of temperature and has the value of 29.13 J/Kmole, calculate the value of the standard molar entropy of N₂(g) at 373K. b. In reality, the molar heat capacity of N₂(g) in the range 200 K to 400 K is given by Cp,m = 28.58 +3.77x10-³T (K-¹) In which the value of Cp,m has units of J/Kmole. Using this relationship, calculate the value of the standard molar entropy of N₂(g) at 373 K.
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![**Exercise on Standard Molar Entropy of Nitrogen**
**1. The value of the standard molar entropy of \( \text{N}_2(g) \) at 298K is 191.6 J/Kmole (Table 2C.7).**
a. If we assume that the value of the heat capacity is independent of temperature and has the value of 29.13 J/Kmole, calculate the value of the standard molar entropy of \( \text{N}_2(g) \) at 373K.
b. In reality, the molar heat capacity of \( \text{N}_2(g) \) in the range 200 K to 400 K is given by:
\[
C_{p,m} = 28.58 + 3.77 \times 10^{-3} T \, (\text{K}^{-1})
\]
Here, the value of \( C_{p,m} \) is in units of J/Kmole. Using this relationship, calculate the value of the standard molar entropy of \( \text{N}_2(g) \) at 373K.
**Explanation:**
This exercise explores the calculation of entropy changes using standard molar entropy values and heat capacity. Part (a) assumes constant heat capacity, while part (b) considers temperature-dependent heat capacity using a given formula.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc944e8dc-d275-4b70-8def-6573a43e5eec%2F63bed64d-c4aa-417f-82e4-1c9ba22db309%2Frqhbo8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Exercise on Standard Molar Entropy of Nitrogen**
**1. The value of the standard molar entropy of \( \text{N}_2(g) \) at 298K is 191.6 J/Kmole (Table 2C.7).**
a. If we assume that the value of the heat capacity is independent of temperature and has the value of 29.13 J/Kmole, calculate the value of the standard molar entropy of \( \text{N}_2(g) \) at 373K.
b. In reality, the molar heat capacity of \( \text{N}_2(g) \) in the range 200 K to 400 K is given by:
\[
C_{p,m} = 28.58 + 3.77 \times 10^{-3} T \, (\text{K}^{-1})
\]
Here, the value of \( C_{p,m} \) is in units of J/Kmole. Using this relationship, calculate the value of the standard molar entropy of \( \text{N}_2(g) \) at 373K.
**Explanation:**
This exercise explores the calculation of entropy changes using standard molar entropy values and heat capacity. Part (a) assumes constant heat capacity, while part (b) considers temperature-dependent heat capacity using a given formula.
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