A gas bulb of $1 L$ capacity contains $2.0 \times 10^{11}$ molecules of nitrogen exerting a pressure of $7.57 \times 10^{3} N m^{- 2}$ . 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.

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A gas bulb of

1 L

capacity contains

2.0 \times 10^{11}

molecules of nitrogen exerting a pressure of

7.57 \times 10^{3} N m^{- 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.

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Text solutionVerified

Answer:

407 m s^{- 1}

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Question Text	A gas bulb of $1 L$ capacity contains $2.0 \times 10^{11}$ molecules of nitrogen exerting a pressure of $7.57 \times 10^{3} N m^{- 2}$ . 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.
Answer Type	Text solution:1
Upvotes	150

Text solutionVerified

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