A 290 ml gas sample contains argon and nitrogen at a temperature of 65 ?c. the total pressure of the sample is 725 mmhg and the

Question

melomori [17]

4 years ago

15

A 290 ml gas sample contains argon and nitrogen at a temperature of 65 ?c. the total pressure of the sample is 725 mmhg and the

partial pressure of argon is 231 mmhg. what mass of nitrogen is present

Chemistry

1 answer:

Anna35 [415] · Answer 1 · 2021-12-06T23:03:37+03:00

The partial pressure of nitrogen in the problem is 725 - 231 = 494 mmHg.
494 / 760 = 0.650 atm. To continue, we will use the ideal gas equation to find the mole of N2 and from that, we can find the mass of N2.

PV = nRT ----> n= PV/RT

Find the mole of Nitrogen
Given P=0.650 atm

n= (0.650)x(255/1000) / (0.082 x 338)
= (0.650) (0.255) / 27.716
= 0.16575 / 27.716
= 0.0060 moles

Find the mass of nitrogen
G= n x Mr (N2)
= 0.0060 x 28
= 0.168 grams

So the mass of nitrogen is 0.168