Calculate the average kinetic energy (unit J) of O2 molecule at 307K. Please enter your answer using scientific notation with 3 significant figures, for example: 2.54E-25.

The average kinetic energy (\(E_k\)) of a gas molecule can be calculated using the formula:

\[
E_k = \frac{3}{2} k_B T
\]

where:
- \(k_B\) is the Boltzmann constant, \(1.38 \times 10^{-23} \, \text{J/K}\),
- \(T\) is the temperature in Kelvin.

Given:
- \(T = 307 \, \text{K}\)

Now, let's calculate the average kinetic energy:

\[
E_k = \frac{3}{2} \times 1.38 \times 10^{-23} \, \text{J/K} \times 307 \, \text{K}
\]

Let's compute this.The average kinetic energy of an \(\text{O}_2\) molecule at 307 K is \(6.35 \times 10^{-21} \, \text{J}\) in scientific notation.

Would you like more details on the calculation, or do you have any other questions?

Here are five related questions you might find interesting:
1. How does the average kinetic energy of a molecule change with temperature?
2. What is the relationship between kinetic energy and the speed of gas molecules?
3. How would the kinetic energy differ if the gas were helium instead of oxygen?
4. What is the significance of the Boltzmann constant in statistical mechanics?
5. How does the kinetic theory of gases explain pressure in a container?

**Tip:** Remember that the kinetic energy of molecules is directly proportional to the absolute temperature, so doubling the temperature would double the average kinetic energy.

Calculate the average kinetic energy (unit J) of an O2 molecule at 307K. Please enter your answer using scientific notation with 3 significant figures, for example: 2.54E-25.

Calculate the average kinetic energy of an O2 molecule at 307K using the kinetic theory of gases. Learn the formula E_k = (3/2) * k_B * T and understand how temperature affects molecular motion. Suitable for students in Grades 11-12.

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