Question

Average kinetic energy of \( H_2 \) molecule at 300K is \( E \). At the same temperature, average kinetic energy of \( O_2 \) molecule will be

• A. \( \frac{E}{2} \)
• B. \( E \)
• C. \( \frac{E}{4} \)
• D. \( \frac{E}{8} \)

Hint:

For ideal gases, the average kinetic energy of molecules depends only on the temperature, not on the type of gas.

Answer 1

The Correct Option is B

Step 1: Understanding the problem.
The average kinetic energy of a gas molecule is given by the equation: \[ KE = \frac{3}{2} k_B T \] where \( k_B \) is Boltzmann's constant and \( T \) is the temperature in Kelvin. The average kinetic energy is the same for all ideal gases at the same temperature, regardless of the type of molecule (whether \( H_2 \), \( O_2 \), or others). Therefore, the average kinetic energy for \( O_2 \) will be the same as for \( H_2 \).
Step 2: Conclusion.
Thus, the average kinetic energy of \( O_2 \) molecule at 300K is \( E \), corresponding to option (B).