The kinetic theory of gases perdicts that total kinetic energy of a gaseous assembly depends on

Pressure of the gas

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Temperature of the gas

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Volume of the gas

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Pressure, volume and temperature of the gas

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Solution

The correct option is B
Temperature of the gas

$K . E = \frac{3}{2} R T$ it means that K.E depends upon T (absolute temperature) only.

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Similar questions

Q. The kinetic theory of gases predicts that total kinetic energy of a gaseous assembly depends on :

According to kinetic theory of gasses at Zero kelvin

a) Pressure of ideal gas is zero

b) Volume of ideal gas is zero

c) Internal energy of ideal gas is zero

d) Matter exists in gaseous state only

Q. In defining the ideal gas temperature scale, it is assumed that the pressure of the gas at constant volume is proportional to the temperature T. How can we verify whether this is true or not? Do we have to apply the kinetic theory of gases? Do we have to depend on experimental result that the pressure is proportional to temperature?

Q. Use kinetic theory of gases to show that the average Kinetic energy of a molecule of an ideal gas is directly proportional to the absolute temperature of the gas.

In the kinetic theory of gases, we try to relate macroscopic properties of a gas, like pressure, volume and temperature to its microscopic properties (properties of each atom or molecule) like particle speeds, momenta, kinetic energies, etc. Which of the following is/are incorrect assumption(s) for building the theory?

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The kinetic theory of gases perdicts that total kinetic energy of a gaseous assembly depends on

The correct option is B Temperature of the gas K.E=32RT it means that K.E depends upon T (absolute temperature) only.

The correct option is B
Temperature of the gas

$K . E = \frac{3}{2} R T$ it means that K.E depends upon T (absolute temperature) only.