A mixture of 7 , g of nitrogen and 11 , g of | vedclass

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(B) The ideal gas equation for the mixture is $P V = n_{mix} R T$. The density of the mixture is given by $\rho = \frac{M_{total}}{V}$. Total mass $M_

Vedclass · Accepted Answer

$1.5$

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(B) The ideal gas equation for the mixture is $P V = n_{mix} R T$. The density of the mixture is given by $ho = \frac{M_{total}}{V}$. Total mass $M_{total} = 7 \, g + 11 \, g = 18 \, g = 18 	imes 10^{-3} \, kg$. Number of moles of $N_2$ $(n_1)$ = $\frac{7}{28} = 0.25 \, mol$. Number of moles of $CO_2$ $(n_2)$ = $\frac{11}{44} = 0.25 \, mol$. Total moles $n_{mix} = n_1 + n_2 = 0.25 + 0.25 = 0.5 \, mol$. Using $V = \frac{n_{mix} R T}{P}$,we have $V = \frac{0.5 	imes 8.314 	imes 290}{1.01 	imes 10^5} \approx 0.01193 \, m^3$. Density $ho = \frac{18 	imes 10^{-3}}{0.01193} \approx 1.508 \, kg/m^3$. Thus,the density is approximately $1.5 \, kg/m^3$.

$A$ mixture of $7 \, g$ of nitrogen and $11 \, g$ of carbon dioxide is kept in a container at a temperature of $T = 290 \, K$. If the pressure of the mixture is $1 \, atm$ $(1.01 \times 10^5 \, N/m^2)$,then the density of the mixture is approximately . . . . . . $kg/m^3$.

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