Answer;
Explanation:
CHECK THE COMPLETE QUESTION BELOW:
chemist is studying the properties of a gas under various conditions. He observes that when the gas is at room temperature and low pressure, it behaves as an ideal gas. When the gas is cooled to 10 kelvin and is placed under high pressure, however, it deviates significantly from an ideal gas. Explain these observations.
ideal gas reffered to as one that has the collisions between its atoms or molecules perfectly eleastic and in which there are no intermolecular attractive forces existing between them. The ideal gas concept is important because it obeys the ideal gas law.
Which is PV=nRT
Where P is the pressure
T is the Temperature
V is the Volume
R is ideal gas constant
n is amount of substance
The ideal gas model assumes that gas particles experience no intermolecular attractions. These are the behavior of gases under different condition
✓At low temperature, gas particles move slowly.
-✓At high pressures, gas particles are very close together.
✓ When the particles of gases are close they have low speed and their low speed allow intermolecular forces to become important at high pressure and low temperature.
OBSERVATION S:
At room temperature which is comfortable ambient temperature, generally taken as about 20°C to 25C
Gases behave non ideally at cold temperatures, So when the gas is cooled to 10Kelvin, molecules are moving relatively slowly past one another, then they give room for the repulsive and/or attractive forces between their molecules giving room for deviation from an Ideal Gas.
The intermolecular forces cause the gas to deviate from ideal behavior So, the reason why a gas deviate from ideal behaviour may be due to some two assumptions of kinetic theory of gases. The forces of attraction between gas molecules are negligible. When the gas is placed under high pressure the gas molecules get more crowded and the amount of empty space between the molecules is reduced.
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