Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
![### Ideal Gas Law Calculation
In this activity, we are applying the Ideal Gas Law equation to determine the number of moles (n) of a gas. The formula for the Ideal Gas Law is given by:
\[ n = \frac{PV}{RT} \]
where:
- \( P \) is the pressure,
- \( V \) is the volume,
- \( R \) is the universal gas constant,
- \( T \) is the temperature in Kelvin.
#### Given Data:
- Pressure (\( P \)): \( 1.25 \) atm
- Volume (\( V \)): \( 0.916 \) L
- Universal Gas Constant (\( R \)): \( 0.082057 \) L·atm/(mol·K)
- Temperature (\( T \)): \( 308.7 \) K
#### Calculation:
Plugging in the given values:
\[
n = \frac{(1.25\ \text{atm})(0.916\ \text{L})}{(0.082057\ \text{L·atm}/\text{mol·K})(308.7\ \text{K})}
\]
### Incorrect Attempt
In this specific example, the student entered \( n = 29 \) mol, which was incorrect. The system allows multiple attempts, and upon rechecking, the correct calculation should be performed as outlined above.
#### User Interface Explanation:
- A text box is provided to input the calculated number of moles.
- "Recheck" button allows the user to verify the entered value.
- "Submit Answer" button for final submission.
- "Try Another Version" button if the user wishes to attempt a different problem.
- The attempt counter indicates that the user has 10 item attempts remaining.
Please make sure to re-evaluate your calculation if you get an incorrect answer, considering the precision of the constants and significant figures involved in the problem.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7fd0ba23-8656-4cc2-b060-9c89e43ba056%2F3550377d-5213-4894-89d8-7f8317fcf778%2Fm5xeqc_processed.jpeg&w=3840&q=75)
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