We’re being asked to calculate the kinetic energy of 1 mol of N_{2} molecules with a speed of 1050 mph.

To calculate for **Kinetic Energy (K.E.)**, we’re going to use the following equation:

$\overline{){\mathbf{K}}{\mathbf{.}}{\mathbf{E}}{\mathbf{.}}{\mathbf{=}}\frac{\mathbf{1}}{\mathbf{2}}{\mathbf{m}}{{\mathbf{v}}}^{{\mathbf{2}}}}$

E_{kinetic energy} = J

m = mass, in kg

v = velocity of the e^{-} = m/s

**We’re going to calculate the Kinetic Energy of N _{2} molecules using the following steps:**

At 20°C (approximately room temperature) the average velocity of N_{2} molecules in air is 1050 mph. What is the total kinetic energy of 1 mol of N_{2} molecules moving at this speed?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Kinetic Energy of Gases concept. You can view video lessons to learn Kinetic Energy of Gases. Or if you need more Kinetic Energy of Gases practice, you can also practice Kinetic Energy of Gases practice problems.

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Our tutors rated the difficulty of*At 20°C (approximately room temperature) the average velocit...*as high difficulty.

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Our expert Chemistry tutor, Dasha took 4 minutes and 47 seconds to solve this problem. You can follow their steps in the video explanation above.

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Based on our data, we think this problem is relevant for Professor Shukla's class at HCC.