### Isothermal and Adiabatic Processes of a Monatomic Ideal Gas#### Problem Statement1. **Initial Conditions:** - **Moles of Gas:** One mole of a monatomic ideal gas - **Initial Pressure (P):** 11 atm - **Initial Volume (V):** 1 L2. **Process Description:** - **Isothermal Expansion:** - The gas expands isothermally to 4 L. - **Adiabatic Expansion:** - Followed by adiabatic expansion to 6 L. - **Isothermal Compression:** - The gas is then compressed isothermally to 1.70 atm. - **Adiabatic Compression:** - Finally, adiabatically compressed back to 1 L.#### Thermodynamic StatesThe table summarizes the state variables through the different stages of the process:| **STATE** | **P (atm)** | **V (L)** | **T (K)** ||-----------|-------------|-----------|-----------|| 1 | 11 | 1 | 134 || 2 | 2.75 | 4 | 134 || 3 | 1.4 | 6 | 102.4 || 4 | 1.7 | 4.94 | 102.4 |#### Exerciseb. **Complete the Following Table:**Calculate the thermodynamic quantities for the given processes using the first law of thermodynamics:- **Q** (Heat Transfer)- **W** (Work Done)- **ΔU** (Change in Internal Energy)- **ΔH** (Change in Enthalpy)- **ΔS** (Change in Entropy)| **Process** | **Q (kJ)** | **W (kJ)** | **ΔU (kJ)** | **ΔH (kJ)** | **ΔS (J/K)** ||-------------|------------|------------|-------------|-------------|--------------|| 1 ➞ 2 | | | | | || 2 ➞ 3 | | | | | || 3 ➞ 4 | | | | | || 4 ➞ 1

Given data, n = No. of moles = 1 mole = 10-3 Kmol we know, n = mM where, m=mass of the ideal gas, M…

1. One mole of a monatomic ideal gas is held at the start at a pressure of 11 atm and 1 L. The gas undergoes isothermal expansion to 4 L followed by adiabatic expansion to 6 L. The gas is then isothermally compressed to 1.70 atm and adiabatically compressed bac to 1 L. STATE P (atm) v (L) т (к) 1 11 1 134 2 2.75 4 134 1.4 6. 102.4 4 1.7 4.94 102.4 b. Complete the table below and show your work. Q (kJ) w (k) AU (kJ) AH (kJ) AS (J/K) Process 10 2 2 0 3 3 0 4 1

1. One mole of a monatomic ideal gas is held at the start at a pressure of 11 atm and 1 L. The gas undergoes isothermal expansion to 4 L followed by adiabatic expansion to 6 L. The gas is then isothermally compressed to 1.70 atm and adiabatically compressed bac to 1 L. STATE P (atm) v (L) т (к) 1 11 1 134 2 2.75 4 134 1.4 6. 102.4 4 1.7 4.94 102.4 b. Complete the table below and show your work. Q (kJ) w (k) AU (kJ) AH (kJ) AS (J/K) Process 10 2 2 0 3 3 0 4 1

Elements Of Electromagnetics

7th Edition

ISBN:9780190698614

Author:Sadiku, Matthew N. O.

Publisher:Sadiku, Matthew N. O.

ChapterMA: Math Assessment

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Concept explainers

Properties of Pure Substances

A substance with fixed chemical composition throughout is called a pure substance like water, air, and nitrogen. A pure substance does not have to be a single element or compound. A mixture of two or more phases of a pure substance is also a pure substance as long as the chemical composition is the same for all phases. These substances mainly have a constant/ uniform composition. The substances also have fixed boiling and melting points. A pure substance takes part in a chemical reaction to form predictable products.

Question

### Isothermal and Adiabatic Processes of a Monatomic Ideal Gas

#### Problem Statement

1. **Initial Conditions:**
- **Moles of Gas:** One mole of a monatomic ideal gas
- **Initial Pressure (P):** 11 atm
- **Initial Volume (V):** 1 L

2. **Process Description:**
- **Isothermal Expansion:**
- The gas expands isothermally to 4 L.
- **Adiabatic Expansion:**
- Followed by adiabatic expansion to 6 L.
- **Isothermal Compression:**
- The gas is then compressed isothermally to 1.70 atm.
- **Adiabatic Compression:**
- Finally, adiabatically compressed back to 1 L.

#### Thermodynamic States

The table summarizes the state variables through the different stages of the process:

| **STATE** | **P (atm)** | **V (L)** | **T (K)** |
|-----------|-------------|-----------|-----------|
| 1 | 11 | 1 | 134 |
| 2 | 2.75 | 4 | 134 |
| 3 | 1.4 | 6 | 102.4 |
| 4 | 1.7 | 4.94 | 102.4 |

#### Exercise

b. **Complete the Following Table:**

Calculate the thermodynamic quantities for the given processes using the first law of thermodynamics:

- **Q** (Heat Transfer)
- **W** (Work Done)
- **ΔU** (Change in Internal Energy)
- **ΔH** (Change in Enthalpy)
- **ΔS** (Change in Entropy)

| **Process** | **Q (kJ)** | **W (kJ)** | **ΔU (kJ)** | **ΔH (kJ)** | **ΔS (J/K)** |
|-------------|------------|------------|-------------|-------------|--------------|
| 1 ➞ 2 | | | | | |
| 2 ➞ 3 | | | | | |
| 3 ➞ 4 | | | | | |
| 4 ➞ 1

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