A two litre flask contains a mixture of 16g of oxygen, 7g of nitrogen and 2g of hydrogen at 20^@C. Report the total pressure and partial pressures.

A two litre flask contains a mixture of 16g of oxygen, 7g of nitrogen

1.	A two litre flask contains a mixture of 16g of oxygen, 7g of nitrogen and 2g of hydrogen at 20^@C. Report the total pressure and partial pressures.
Answer» <html><body><p></p>Solution :Total number of moles of mixture ` = (16g " of"O_(2))/(32g"<a href="https://interviewquestions.tuteehub.com/tag/mol-1100196" style="font-weight:bold;" target="_blank" title="Click to know more about MOL">MOL</a>"^(-<a href="https://interviewquestions.tuteehub.com/tag/1-256655" style="font-weight:bold;" target="_blank" title="Click to know more about 1">1</a>)) + (7g "of" N_(2))/(28 g"mol"^(-1)) + (1g "of" H_(2))/(2g "mol"^(-1))` <br/> Total number of moles ` = (1)/(2) + (1)/(4)+ 1 = (<a href="https://interviewquestions.tuteehub.com/tag/7-332378" style="font-weight:bold;" target="_blank" title="Click to know more about 7">7</a>)/(4)` <br/> <a href="https://interviewquestions.tuteehub.com/tag/using-7379753" style="font-weight:bold;" target="_blank" title="Click to know more about USING">USING</a> ideal gas equation, `P = n (RT)/(V) = (7)/(4) xx (0.0821 xx 293)/(2) =21` atm <br/> Partial pressure of oxygen ` = P_(O_(2)) = ("number moles of " O_(2))/("total number of moles") xx "pressure" = (1)/(2) xx (4)/(7) xx 21 = 6` atm <br/> Similarly, `P_(N_(2)) = (1)/(4) xx (4)/(7) xx 21 = 3` atm <br/> Similarly, `P_(H_(2)) = (1)/(1) xx (4)/(7) xx 21 = 12` atm</body></html>