What Is the RMS Speed of a Nitrogen Molecule at 35°C?

AI Thread Summary
The discussion focuses on calculating the root mean square (rms) speed of a nitrogen molecule at 35°C using the formula V(rms) = sqrt((3RT)/M). The user initially calculated the rms speed as 23.4 m/s but received an incorrect response from their online homework system. It was noted that the mass should be converted from grams to kilograms, as nitrogen is a diatomic molecule, which affects the calculations. Additionally, participants discussed the mass of nitrogen molecules and the implications for the calculations. The importance of unit conversion and understanding molecular mass in the context of the problem was emphasized.
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Homework Statement



Compute the rms speed of a nitrogen molecule of 35.0 celcius.

Homework Equations



V(rms) = sqrt((3RT)/M)

The Attempt at a Solution



I plugged in 8.31 for R and 308 K for T and 14.0 g/mol for M. I arrived at a solution of 23.4 m/s but this answer came back as incorrect in online homework. However, I used this value to complete parts b and c to this question and correctly completed them. What gives?
 
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Did you change g to Kg?
 
A couple of questions to ponder:

(a) If 1 mole of nitrogen atoms has a mass of 14.0 g, then a mole of nitrogen molecules has a mass of ____?

(b) If 1 mole of nitrogen molecules has a mass of (insert answer to a here), then a single nitrogen molecule has a mass of ____?

Also, as Dadface said, convert from g to kg.
 
Nitrogen is a diatomic molecule. Thanks for the reminder...all is well.
 

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