2 , g of {O_2} gas is taken at 27^{circ}C and | vedclass

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(A) Given: Mass of ${O_2}$ $(m)$ = $2 \, g$,Temperature $(T)$ = $27^{\circ}C = 300 \, K$,Pressure $(P)$ = $76 \, cm$ of $Hg = 1 \, atm = 1.013 	imes

Vedclass · Accepted Answer

$1.53$

Vedclass · Answer

(A) Given: Mass of ${O_2}$ $(m)$ = $2 \, g$,Temperature $(T)$ = $27^{\circ}C = 300 \, K$,Pressure $(P)$ = $76 \, cm$ of $Hg = 1 \, atm = 1.013 	imes 10^5 \, Pa$.Using the Ideal Gas Equation: $PV = nRT = \frac{m}{M}RT$.Here,$M$ (molar mass of ${O_2}$) = $32 \, g/mol$ and $R = 0.0821 \, L \cdot atm \cdot K^{-1} \cdot mol^{-1}$.$V = \frac{mRT}{MP} = \frac{2 	imes 0.0821 	imes 300}{32 	imes 1} = \frac{49.26}{32} \approx 1.54 \, L$.Using $R = 8.314 \, J \cdot K^{-1} \cdot mol^{-1}$ and $P = 1.013 	imes 10^5 \, Pa$:$V = \frac{(2/32) 	imes 8.314 	imes 300}{1.013 	imes 10^5} = 0.001539 \, m^3 = 1.539 \, L$.Rounding to the nearest option,the correct answer is $1.53 \, L$.

$2 \, g$ of ${O_2}$ gas is taken at $27^{\circ}C$ and a pressure of $76 \, cm$ of $Hg$. Find the volume of the gas (in liters).

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