Why Is a gas at 1.3 atm pressure and 20 L volume, at -10 degrees Celsius and 1 mole the gas not ideal?
To determine whether a gas is ideal or not, we need to consider whether it follows the ideal gas law equation, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
In the given scenario, the gas is at a pressure of 1.3 atm and a volume of 20 L. However, it is stated that the temperature is -10 degrees Celsius. To use the ideal gas law, we need to convert the temperature to Kelvin by adding 273.15.
T = -10 + 273.15 = 263.15 K
Now, let's consider the conditions for an ideal gas:
1. The particles of the gas do not interact with each other.
2. The volume of the gas particles is negligible compared to the volume of the container they are in.
3. There are no intermolecular forces acting between the gas particles.
If any of these conditions are violated, the gas will not behave ideally.
In this case, we are only provided with the temperature, pressure, volume, and number of moles of the gas. We do not have any information about the nature of the gas or any potential intermolecular interactions. Therefore, we cannot definitively determine whether the gas is ideal or not based on the given information.