A chemical 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.

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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Ideal gas explains the property of gas that has no inter-molecular attractions irrespective of temperature and pressure.

Explanation:

Ideal gases assumes that the gases would experience no inter-molecular attraction and collision with other gases.

These gases are perfectly exhibiting elastic collision in nature.

The particle of gases moves slowly at lower temperature and the gases would become close when they exhibit high pressure.

The "closeness of the gas-particle" and "low-speed characteristics" are the important observations noted.

The inter-molecular forces deviate the property of gases from ideal gas behavior.

Step-by-step explanation:

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step-by-step explanation:

the required function is .

step-by-step explanation:

from the given table it is noticed that the graph passing through (-3,7), (0,4), (3,1) and (8,-4).

it is a linear function because the value of y is decrease by one as the value of x increase by 1.

the slope of the function is

the slope of the function is -1 and the y-intercept is 4.

the slope intercept form is

where, m is slope and b is y-intercept.

therefore the required function is . the graph of this function is shown below.