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Q. A $10.0 \,L$ flask contains $64\, g$ of oxygen at $27^{\circ} C$. (Assume $O _{2}$ gas is behaving ideally). The pressure inside the flask in bar is (Given $R =0.0831 \,L\, bar\, K ^{-1} mol ^{-1}$ )

NEETNEET 2022States of Matter

Solution:

$V =10 L $
$ W _{ O _{2}}=64 \,g$
$T =2{ }^{\circ} C$
$ n _{ O _{2}}=2$
$R =0.083 . L$ bar $K ^{-1} \,mol ^{-1}$
Ideal gas equation $PV = nRT$
$P =\frac{2 \times 0.0831 \times 300}{10}$
$P =4.9$ bar