Explanation
Kinetic energy of ideal gas depends only on its temperature. Hence, it remains constant whether pressure is increased or decreased.
Kinetic energy is directly proportional to temperature. Hence if temperature is doubled, kinetic energy will also be doubled.
Average translational K.E. of a molecules = 3/2 kBT (Where, kB = Boltzmann's constant ) This is same, for all gases at same temperature.
A monoatomic gas molecule has only three translational degrees of freedom.
A diatomic molecule has three translational and two rotational degrees of freedom. Hence total degrees of freedom, f = 3 + 2 = 5.
For an ideal gas PV = constant i.e PV doesn't vary with V.
In isothermal changes, temperature remains constant.
S.I. unit of R is J/mol-K.
Molecules of ideal gas behaves like perfectly elastic rigid sphere.
From Andrew's curve
The collision of molecules of ideal gas is elastic collision.
At open end phase of pressure wave change by it, so high pressure pulse gets reflected as a low pressure pulse. While at closed end phase of pressure wave does not. change, so high pressure pulse gets reflected again as a high pressure pulse.
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