[" A gas bulb of "1L" capacity contains "2.0times10^(21)" molecules of "],[" nitrogen exerting a pressure of "7.57times10^(3)Nm^(-2)" .Calculate "]

A gas bulb of 1L capacity contains 2.0xx10^(21) molecules of nitrogen exerting a pressure of 7.57xx10^(3)N*m^(-2) . Calculate the rms velocity and temperature off the gas. If ratio of most probable speed to the root mean square speed in 0.82, calculate the most probable speed of the molecules at this temperature.

A gas bulb of 1 litre capacity contains 2.0xx10^(21) molecules of nitrogen exerting a pressure of 7.57xx10^(3)" N "m^(-2) . Calculate the root mean square (r.m.s) speed and the temperature of the gas molecules.

A gas bulb of 1 L capacity contains 2.0xx10^(11) molecules of nitrogen exerting a pressure of 7.57xx10^(3)Nm^(-2) . Calculate the root mean square (rms) speed and the temperature of the gas molecules. If the ratio of the most probable speed to the root mean square is 0.82 , calculate the most probable speed for these molecules at this temperature.

A gas bulb of 1 L capacity contains 2.0xx10^(11) molecules of nitrogen exerting a pressure of 7.57xx10^(3)Nm^(-2) . Calculate the root mean square (rms) speed and the temperature of the gas molecules. If the ratio of the most probable speed to the root mean square is 0.82 , calculate the most probable speed for these molecules at this temperature.

A gas bulb of 1 L capacity contains 2.0xx10^(11) molecules of nitrogen exerting a pressure of 7.57xx10^(3)Nm^(-2) . Calculate the root mean square (rms) speed and the temperature of the gas molecules. If the ratio of the most probable speed to the root mean square is 0.82 , calculate the most probable speed for these molecules at this temperature.

A gas bulb of 1 L capacity contains 2.0xx10^(11) molecules of nitrogen exerting a pressure of 7.57xx10^(3)Nm^(-2) . Calculate the root mean square (rms) speed and the temperature of the gas molecules. If the ratio of the most probable speed to the root mean square is 0.82 , calculate the most probable speed for these molecules at this temperature.

A gas bulb of 1 litre capacity contains 2.0 xx 10^(21) molecules of nitrogen exerting a pressure of 7.57 xx 10^3 Nm^(-2) . Calculate the root mean square speed and the temperature of gas molecules. If the ratio of most probable speed to the root mean square speed is 0.82, calculate the most probable speed for the molecules at this temperature.