Question

If v1 is the speed of sound in a diatomic gas at 273 degree C and v2 is the r.m.s speed of its molecules at 273 K,then v1/v2

Answer 1

Answer:

Explanation:take speed of sound in a diatomic gas and rms speed of molecules and devide

Answer 2

Answer:

$\frac{v_{1} }{v_{2} } =\sqrt{\frac{14}{15} }$

Explanation:

Gases are composed of atoms or molecules that move at different speeds in random directions. Root mean square velocity (RMS velocity) is a way to find a single velocity value for a particle. The average velocity of a gas particle is found using the root mean square velocity formula.

The RMS calculation gives you the root mean square speed, not speed. This is because velocity is a vector quantity that has magnitude and direction. The RMS calculation only gives magnitude or speed. To complete the other tasks, you need to convert the temperature to kelvin and find the molar mass in kg.

We examined pressure and temperature based on their macroscopic definitions. Pressure is force divided by the area on which the force acts, and temperature is measured with a thermometer. We can better understand pressure and temperature from the kinetic theory of gases, a theory that relates the macroscopic properties of gases to the motion of the molecules that make them up. First, we make two assumptions about the molecules in an ideal gas.

There are a very large number N of molecules, all identical, and each of mass m.

Molecules follow Newton's laws and are in continuous motion that is random and isotropic, i.e. the same in all directions.

To derive the ideal gas law and the relationship between microscopic quantities, such as the energy of a typical molecule, and macroscopic quantities, such as temperature, we analyze a sample of an ideal gas in a fixed container, about which we make two additional assumptions:

The molecules are much smaller than the average distance between them, so their total volume is much smaller than the volume of their container (which has volume V). In other words, we consider the van der Waals constant b, the volume of a mole of gas molecules, to be negligible compared to the volume of a mole of gas in the container.

The molecules form perfectly elastic collisions with the walls of the container and with each other. Other forces on them, including gravity and attraction represented by the Van der Waals constant a, are negligible (as required for the assumption of isotropy).

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