How many grams of zinc are required to produc | vedclass

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(A) The balanced chemical equation is: $Zn + H_2SO_4 	o ZnSO_4 + H_2$ At $STP$,$1 \ mol$ of any gas occupies $22400 \ mL$. Therefore,$224 \ mL$ of $H

Vedclass · Accepted Answer

$0.65$

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(A) The balanced chemical equation is: $Zn + H_2SO_4 	o ZnSO_4 + H_2$ At $STP$,$1 \ mol$ of any gas occupies $22400 \ mL$. Therefore,$224 \ mL$ of $H_2$ corresponds to: $n(H_2) = \frac{224 \ mL}{22400 \ mL/mol} = 0.01 \ mol$ From the stoichiometry of the reaction,$1 \ mol$ of $Zn$ produces $1 \ mol$ of $H_2$. So,$0.01 \ mol$ of $Zn$ is required. Mass of $Zn = n 	imes 	ext{molar mass} = 0.01 \ mol 	imes 65 \ g/mol = 0.65 \ g$.

How many grams of zinc are required to produce $224 \ mL$ of hydrogen from dilute $H_2SO_4$ at $STP$?

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