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Is a gas at 1.4 atm pressure and 15 L volume, at -10 degrees Celsius and 1 mole the gas, an ideal gas, why or why not
To determine if a gas is an ideal gas, we can consider the following assumptions of the ideal gas law:
1. The gas particles are assumed to have negligible volume.
2. The gas particles are assumed to have no intermolecular forces.
3. The gas particles are assumed to undergo perfectly elastic collisions.
4. The gas particles are assumed to be in continuous random motion.
Using these assumptions, let's evaluate the given conditions:
1. The pressure of the gas is 1.4 atm, and the volume is 15 L.
- This is within the range of normal pressures and volumes encountered by gases, so it does not violate the assumptions for an ideal gas.
2. The temperature of the gas is -10 degrees Celsius or 263 Kelvin.
- Negative temperatures are not expected, but since ideal gas behavior is not solely dependent on temperature, this does not necessarily disqualify the gas from being ideal.
3. The gas contains 1 mole of gas particles.
- The number of particles is not a determining factor for ideal gas behavior, so this does not affect the conclusion.
Based on the given information, it is not possible to definitively conclude whether the gas behaves as an ideal gas or not. Additional information, such as experimental deviation from ideal gas behavior or knowledge of the specific gas being considered, would be required for a more accurate assessment.