What would be the mass of $10$ L oxygen (molar mass $= 32$ ) at $37^{o}$ C and $70$ cm pressure? Calculate the number of moles of oxygen.

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Solution

Volume $= 10 L = 10^{- 2} m^{3}$
temperature $= 37^{o} C = 310 k$
pressure $= 70 c m$ of $H g = (1 a t m) \times \frac{70}{76} = 0.921 a t m$
ideal gas equation $\Rightarrow p x = n R T$
$(0.921) (1.013 \times 10^{5} P a) (10^{- 2} m^{3}) = (\frac{m}{32}) (8.314) (310)$
$∴$ mass of $10 L$ oxygen, $m = 11.584$ grams
number of modes $n = \frac{m}{M}$
$= \frac{11.584}{32}$
$= 0.3620$ modes
$\Rightarrow ∴$ No. of modes of oxygen is $0.362$ modes

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What would be the mass of 10L oxygen (molar mass =32) at 37oC and 70 cm pressure? Calculate the number of moles of oxygen.

Volume =10 L=10−2m3temperature =37oC=310 kpressure =70 cm of Hg=(1 atm)×7076=0.921 atmideal gas equation ⇒ px=nRT(0.921)(1.013×105 Pa)(10−2m3)=(m32)(8.314)(310)∴ mass of 10 L oxygen, m=11.584 gramsnumber of modes n=mM=11.58432=0.3620 modes⇒ ∴ No. of modes of oxygen is 0.362 modes

What would be the mass of $10$ L oxygen (molar mass $= 32$ ) at $37^{o}$ C and $70$ cm pressure? Calculate the number of moles of oxygen.