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.

Explanation

To solve the problem step by step, we will follow these steps:

### Step 1: Convert Volume to Cubic Meters
Given the volume of the gas bulb is `1 L`, we need to convert it to cubic meters.
\[ \text{Volume} = 1 \, \text{L} = 1 \times 10^{-3} \, \text{m}^3 \]

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