If the pressure, temperature, and amount of gas are kept constant, would the volume of the gas be different if the gas was argon instead of another ideal gas?

• A. No, the volume would be the same because the ideal gas law does not depend on the identity of the gas.
• B. No, the volume would be the same only if the gas is diatomic.
• C. Yes, the volume would be different because argon is a noble gas.
• D. Yes, the volume would be different because argon atoms are heavier than other gases.

Answer: (A)

Verified step by step guidance

1. Recall the Ideal Gas Law, which is given by the equation \(P \times V = n \times R \times T\), where \(P\) is pressure, \(V\) is volume, \(n\) is the amount of gas in moles, \(R\) is the ideal gas constant, and \(T\) is temperature.
2. Note that in the Ideal Gas Law, the volume \(V\) depends only on the pressure \(P\), the amount of gas \(n\), the temperature \(T\), and the constant \(R\). It does not include any term related to the identity or type of gas.
3. Since the problem states that pressure, temperature, and amount of gas are kept constant, these variables do not change regardless of the gas used.
4. Understand that the Ideal Gas Law treats all gases as ideal, meaning their particles do not interact and have no volume themselves, so the volume occupied depends only on \(P\), \(n\), and \(T\), not on the gas's molecular weight or atomic nature.
5. Therefore, the volume of argon gas under these conditions would be the same as the volume of any other ideal gas under the same pressure, temperature, and amount.