Question

One half mole each of nitrogen, oxygen and carbon dioxide are mixed in enclosure of volume $5$ litres and temperature ${27}^o$C. The pressure exerted by mixture is $(R=8.31Jmo{l}^{-1}{K}^{-1})$

• A. $7.48\times {10}^5$N $m^{-2}$
• B. $4\times {10}^5$N $m^{-2}$
• C. $6\times {10}^5$N $m^{-2}$
• D. $3\times {10}^5$N $m^{-2}$

Answer 1

The correct option is A $7.48\times {10}^5$N $m^{-2}$

Using, Dalton's law of partial pressure, $P=P_1+P_2+P_3$
$=\frac{nRT}{V}=\frac{nRT}{V}+\frac{nRT}{V}$
$=\frac{3nRT}{V}$ .(i)
Here, $n=\frac{1}{2},T={27}^{o}C=27+273=300K$
$V=5\times {10}^{-3}{m}^3$

$\therefore P=\frac{3\times 8.31\times 300}{2\times 5\times {10}^{-3}},$ $P=7.48\times {10}^5$N $m^{-2}$