The nitrogen gas pressure inside a container | vedclass

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(D) Given:Pressure of $N_2$ gas $(P) = 2.3 \ atm$Volume $(V) = 2.6 \ cm^3 = 2.6 	imes 10^{-3} \ L$Temperature $(T) = 27^{\circ} C + 273 = 300 \ K$Gas

Vedclass · Accepted Answer

$2 	imes 10^{-4}$

Vedclass · Answer

(D) Given:Pressure of $N_2$ gas $(P) = 2.3 \ atm$Volume $(V) = 2.6 \ cm^3 = 2.6 	imes 10^{-3} \ L$Temperature $(T) = 27^{\circ} C + 273 = 300 \ K$Gas constant $(R) = 0.0821 \ L \ atm \ mol^{-1} \ K^{-1}$Using the ideal gas equation: $PV = nRT$$n = \frac{PV}{RT}$$n = \frac{2.3 \ atm 	imes 2.6 	imes 10^{-3} \ L}{0.0821 \ L \ atm \ mol^{-1} \ K^{-1} 	imes 300 \ K}$$n = \frac{5.98 	imes 10^{-3}}{24.63} \ mol$$n \approx 2.42 	imes 10^{-4} \ mol$Rounding to the nearest provided option, the value is $2 	imes 10^{-4} \ mol$.

The nitrogen gas pressure inside a container of volume $2.6 \ cm^3$ is $2.3 \ atm$ at $27^{\circ} C$. The approximate number of moles of nitrogen present in the container is $[R=0.0821 \ L \ atm \ mol^{-1} \ K^{-1}]$

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