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Stoichiometric Calculations

The weight of...

Question

The weight of $N a C l$ decomposed by $4.9 g$ of $H_{2} S O_{4}$ , if $6 g$ of sodium hydrogen sulphate and $1.825 g$ of $H C l$ , were produced in the reaction is:

6.921 g

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4.65 g

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2.925 g

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1.4 g

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Solution

The correct option is A $2.925 g$
$N a C l + H_{2} S O_{4} \to N a H S O_{4} + H C l$
Given Mass: $x$ $4.9 g$ $6 g$ $1.825 g$
Molecular weight: $58.5 g$ $98 g$ $120 g$ $36.5 g$
Moles: $\frac{x}{58.5}$ $0.05$ $0.05$ $0.05$
Therefore, $0.05$ moles of reactant are reacting produce $0.05$ moles of each of the product.
Therefore, Amount of $N a C l$ consumed: $\frac{x}{58.5} = 0.05$
$x = 2.925 g$

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