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NEET2026PhysicsChapterActual

A sealed container holds a gaseous mixture of Neon ( Ne ), Oxygen ( O₂ ), and Carbon dioxide ( CO₂ ) in thermal equilibrium at a constant temperature. Which of the following statements is correct regarding the root mean square (rms) speed of the molecules in this mixture?

Options

  1. AThe rms speed of CO₂ molecules is the greatest.
  2. BAll molecules have the same rms speed because the mixture is in thermal equilibrium.
  3. CThe rms speed of Neon molecules is the greatest.
  4. DThe rms speed of Oxygen molecules is less than that of CO₂ molecules.

Correct answer

C. The rms speed of Neon molecules is the greatest.

Step-by-step solution

The root mean square (rms) speed of gas molecules is given by the formula: v_ rms = 3RT M where R is the universal gas constant, T is the absolute temperature, and M is the molar mass of the gas. Since the gaseous mixture is in thermal equilibrium, the temperature T is the same for all the gases. Therefore, the rms speed is inversely proportional to the square root of the molar mass: v_ rms 1 M The molar masses of the given gases are: M_ Ne = 20 g/mol M_ O₂ = 32 g/mol M_ CO₂ = 44 g/mol Comparing the molar masses: M

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