A synthetic mixture of nitrogen and Argon has a density of 1.4 g L^(-1) at 0^@C. Calculate the average molecular weight. Find out the volume percentage of nitrogen in the mixture.

A synthetic mixture of nitrogen and Argon has a density of 1.4 g L^(-1

1.	A synthetic mixture of nitrogen and Argon has a density of 1.4 g L^(-1) at 0^@C. Calculate the average molecular weight. Find out the volume percentage of nitrogen in the mixture.
Answer» <html><body><p></p>Solution :Molecular weight (M) can be obtained from density (d) as, `M=(dRT)/(P )` <br/> Average molecular weight of the mixture =` (1.4 xx 0.0821 xx 273 )/(1) = 31.4` <br/> If the % <a href="https://interviewquestions.tuteehub.com/tag/volume-728707" style="font-weight:bold;" target="_blank" title="Click to know more about VOLUME">VOLUME</a> of `N_2 ` is .x. <br/> ` 31.4 = ( x xx 28+(100-x)40)/( 100 )implies12 x = <a href="https://interviewquestions.tuteehub.com/tag/840-1928616" style="font-weight:bold;" target="_blank" title="Click to know more about 840">840</a> orx=70` <br/> The volume <a href="https://interviewquestions.tuteehub.com/tag/percentage-13406" style="font-weight:bold;" target="_blank" title="Click to know more about PERCENTAGE">PERCENTAGE</a> of `N_2` in the mixture = 70</body></html>