What volume of Hydrogen gas,at 273 K and 1 | vedclass

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(C) The balanced chemical equation for the reduction of boron trichloride by hydrogen is:$2BCl_3(g) + 3H_2(g) 	o 2B(s) + 6HCl(g)$First,calculate the

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$67.2$

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(C) The balanced chemical equation for the reduction of boron trichloride by hydrogen is:$2BCl_3(g) + 3H_2(g) 	o 2B(s) + 6HCl(g)$First,calculate the number of moles of Boron $(B)$ produced:$n(B) = \frac{	ext{mass}}{	ext{atomic mass}} = \frac{21.6 \ g}{10.8 \ g/mol} = 2 \ mol$From the stoichiometry of the reaction,$2 \ mol$ of $B$ are produced by $3 \ mol$ of $H_2$ gas.Since $2 \ mol$ of $B$ are produced,the moles of $H_2$ required is $3 \ mol$.At $STP$ ($273 \ K$ and $1 \ atm$),$1 \ mol$ of any ideal gas occupies $22.4 \ L$.Therefore,the volume of $H_2$ required is:$V = 3 \ mol 	imes 22.4 \ L/mol = 67.2 \ L$

What volume of Hydrogen gas,at $273 \ K$ and $1 \ atm$ pressure,will be consumed in obtaining $21.6 \ g$ of elemental boron (atomic mass $= 10.8$) from the reduction of boron trichloride by Hydrogen? (Answer in $L$)

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