How many grams of NaCl are decomposed by 4.9 | vedclass

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(C) The balanced chemical equation is: $NaCl + H_2SO_4 \rightarrow NaHSO_4 + HCl$From the stoichiometry:$1 \ mol$ of $NaCl$ $(58.5 \ g)$ reacts with $

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$2.925$

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(C) The balanced chemical equation is: $NaCl + H_2SO_4 ightarrow NaHSO_4 + HCl$From the stoichiometry:$1 \ mol$ of $NaCl$ $(58.5 \ g)$ reacts with $1 \ mol$ of $H_2SO_4$ $(98 \ g)$ to produce $1 \ mol$ of $NaHSO_4$ $(120 \ g)$ and $1 \ mol$ of $HCl$ $(36.5 \ g)$.Given that $1.825 \ g$ of $HCl$ is produced,which is $\frac{1.825}{36.5} = 0.05 \ mol$.According to the stoichiometry,$0.05 \ mol$ of $H_2SO_4$ is required,which is $0.05 	imes 98 = 4.9 \ g$.Similarly,the amount of $NaCl$ required is $0.05 \ mol 	imes 58.5 \ g/mol = 2.925 \ g$.

How many grams of $NaCl$ are decomposed by $4.9 \ g$ of $H_2SO_4$ to produce sodium hydrogen sulfate and $1.825 \ g$ of $HCl$? $[Na = 23, Cl = 35.5, S = 32, H = 1, O = 16]$

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