What volume of H_2 gas in liters at 1 , text{ | vedclass

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(C) The balanced chemical equation for the reduction of boron trichloride is: $BCl_3 + \frac{3}{2}H_2 \rightarrow B + 3HCl$ Calculate the moles of bor

Vedclass · Accepted Answer

$67.2$

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(C) The balanced chemical equation for the reduction of boron trichloride is: $BCl_3 + \frac{3}{2}H_2 ightarrow B + 3HCl$ Calculate the moles of boron $(B)$ produced: $n(B) = \frac{21.6 \, g}{10.8 \, g/mol} = 2 \, mol$ From the stoichiometry of the reaction,$1 \, mol$ of $B$ requires $\frac{3}{2} \, mol$ of $H_2$. Therefore,$2 \, mol$ of $B$ requires $2 	imes \frac{3}{2} = 3 \, mol$ of $H_2$. At $STP$ ($1 \, 	ext{atm}$,$273 \, K$),the volume of $1 \, mol$ of gas is $22.4 \, L$. Volume of $H_2 = 3 \, mol 	imes 22.4 \, L/mol = 67.2 \, L$.

What volume of $H_2$ gas in liters at $1 \, \text{atm}$ pressure and $273 \, K$ temperature is required to reduce $21.6 \, g$ of boron trichloride $(BCl_3)$ (atomic weight of $B = 10.8$) to obtain boron?

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