A 10.0 , L flask contains 64 , g of oxygen at | vedclass

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(C) Given:Volume $V = 10.0 \, L$Mass of $O_2$ $(W)$ = $64 \, g$Molar mass of $O_2$ $(M)$ = $32 \, g \, mol^{-1}$Temperature $T = 27^{\circ} C = 27 + 2

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$4.9$

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(C) Given:Volume $V = 10.0 \, L$Mass of $O_2$ $(W)$ = $64 \, g$Molar mass of $O_2$ $(M)$ = $32 \, g \, mol^{-1}$Temperature $T = 27^{\circ} C = 27 + 273 = 300 \, K$Gas constant $R = 0.0831 \, L \, bar \, K^{-1} \, mol^{-1}$Step $1$: Calculate the number of moles $(n)$:$n = \frac{W}{M} = \frac{64 \, g}{32 \, g \, mol^{-1}} = 2 \, mol$Step $2$: Use the ideal gas equation $PV = nRT$ to find pressure $(P)$:$P = \frac{nRT}{V}$$P = \frac{2 \, mol 	imes 0.0831 \, L \, bar \, K^{-1} \, mol^{-1} 	imes 300 \, K}{10.0 \, L}$$P = \frac{49.86}{10} \, bar = 4.986 \, bar \approx 4.9 \, bar$

$A$ $10.0 \, L$ 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 $R = 0.0831 \, L \, bar \, K^{-1} \, mol^{-1}$)

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$A$ $10.0 \, L$ 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 $R = 0.0831 \, L \, bar \, K^{-1} \, mol^{-1}$)