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 molecule in a gas can be calculated using the following 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 (\(307 \, \text{K}\)).

Let's calculate the average kinetic energy.The average kinetic energy of an \(O_2\) molecule at 307 K is \(6.35 \times 10^{-21}\) J.

Would you like more details or have any questions about this calculation?

Here are 5 related questions you might find interesting:
1. How does the average kinetic energy of \(O_2\) molecules change if the temperature is increased to 500 K?
2. What would be the average kinetic energy of an \(N_2\) molecule at 307 K?
3. How does the kinetic energy relate to the speed of the molecules?
4. What is the relationship

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.

Learn how to calculate the average kinetic energy of an O2 molecule at 307K using the kinetic theory of gases. This example uses the formula E_k = (3/2) * k_B * T, with step-by-step guidance suitable for students in Grades 11-12.

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