2 g of O_2 at 27 ^circ C and 760 mm of Hg | vedclass

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(A) Given: Mass of $O_2$ $(w)$ = $2 \ g$,Molar mass of $O_2$ $(M)$ = $32 \ g/mol$,Temperature $(T)$ = $27 + 273 = 300 \ K$,Pressure $(P)$ = $760 \ mm

Vedclass · Accepted Answer

$1.5$

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(A) Given: Mass of $O_2$ $(w)$ = $2 \ g$,Molar mass of $O_2$ $(M)$ = $32 \ g/mol$,Temperature $(T)$ = $27 + 273 = 300 \ K$,Pressure $(P)$ = $760 \ mm \ Hg = 1 \ atm$.Using the ideal gas equation: $PV = nRT$.Number of moles $(n)$ = $\frac{w}{M} = \frac{2}{32} = 0.0625 \ mol$.Substituting values into the equation: $V = \frac{nRT}{P} = \frac{0.0625 	imes 0.0821 	imes 300}{1}$.$V = 1.539 \ L \approx 1.5 \ L$.

$2 \ g$ of $O_2$ at $27 \ ^\circ C$ and $760 \ mm$ of $Hg$ pressure has volume ............. $L$.

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