A sample of 0.125 g of an organic compound w | vedclass

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(A) Step $1$: Calculate the pressure of dry $N_2$ gas.$P_{N_2} = P_{total} - P_{H_2O} = 759 \ mm \ Hg - 14.2 \ mm \ Hg = 744.8 \ mm \ Hg$.Step $2$: Co

Vedclass · Accepted Answer

$22$

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(A) Step $1$: Calculate the pressure of dry $N_2$ gas.$P_{N_2} = P_{total} - P_{H_2O} = 759 \ mm \ Hg - 14.2 \ mm \ Hg = 744.8 \ mm \ Hg$.Step $2$: Convert units to standard values.$P = \frac{744.8}{760} \ atm$,$V = \frac{22.78}{1000} \ L$,$T = 280 \ K$,$R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$.Step $3$: Calculate moles of $N_2$ using the ideal gas equation $PV = nRT$.$n_{N_2} = \frac{PV}{RT} = \frac{744.8 	imes 22.78}{760 	imes 0.082 	imes 280 	imes 1000} \approx 0.000971 \ mol$.Step $4$: Calculate mass of $N_2$ and percentage.$Mass_{N_2} = 0.000971 	imes 28 \ g/mol = 0.027188 \ g$.$\%N = \frac{Mass_{N_2}}{Mass_{sample}} 	imes 100 = \frac{0.027188}{0.125} 	imes 100 \approx 21.75\%$.The nearest integer is $22$.

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