A sample of argon gas has a volume of 735 mL at a pressure of 1.20 atm and a temperature of 112 °C. What is the final volume of the gas, in milliliters, when the pressure and temperature of the gas sample are changed to the following, if the amount of gas does not change? You may want to reference (Pages 289 - 290) Section 8.5 while completing this problem.
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.
![**Gas Laws Application: Volume Calculation**
A sample of argon gas has a volume of 735 mL at a pressure of 1.20 atm and a temperature of 112°C. What is the final volume of the gas, in milliliters, when the pressure and temperature of the gas sample are changed to the following, if the amount of gas does not change?
You may want to reference [Pages 289 - 290] Section 8.5 while completing this problem.
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**Explanation:**
The problem is likely related to the ideal gas law or combined gas law, where you need to adjust the volume of a gas based on changes in temperature and pressure while keeping the amount of gas constant. Calculations will involve using formulas to determine the final volume under the new conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fec34e07b-01ec-4806-810c-ebd28802db2a%2F4a5adf64-f527-40be-9cba-4e0eb9a3a542%2Fll87c44_processed.jpeg&w=3840&q=75)
![### Part C
14.9 atm and -13°C
Express your answer with the appropriate units.
\[ V = \text{Value} \quad \text{Units} \]
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Multiplying the initial and final pressure values together would result in units of atm². Rearrange the combined gas law to solve for the final volume \( V_2 \):
\[ \frac{P_1 \times V_1}{T_1} = \frac{P_2 \times V_2}{T_2} \]
Where:
- \( P_1 \) is the initial pressure,
- \( V_1 \) is the initial volume,
- \( T_1 \) is the initial temperature,
- \( P_2 \) is the final pressure,
- \( T_2 \) is the final temperature.
All temperature values must be in kelvins to use this equation.
You may need to review [Rearrangement of Equations Involving Multiplication and Division](#).
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