How much faster does nitrogen monoxide (NO) effuse in comparison to dinitrogen tetraoxide (N2O4)?

The answer to this problem is nitrogen monoxide effuses approximately 1.75 times faster than dinitrogen tetroxide

Explanation:

I got this answer by finding out the molar masses of both substances (NO's molar mass=30 G/mol and N2O4's molar mass= 92 G/mol) and I divided the square roots of these numbers (remember to always have the larger molar mass as the numerator or number on top of your fraction) and the square root of 92 divided by the square root of 30 is equal to approximately 1.75. So therefore, NO diffuses 1.75x faster than N2O4 (the gas with the smaller molar mass always diffuses faster)