How many grams of ethanol are required to obt | vedclass

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(C) The chemical reaction between ethanol and sodium metal is: $2C_2H_5OH + 2Na \rightarrow 2C_2H_5ONa + H_2$ From the stoichiometry,$2 \ mol$ of etha

Vedclass · Accepted Answer

$1.15$

Vedclass · Answer

(C) The chemical reaction between ethanol and sodium metal is: $2C_2H_5OH + 2Na ightarrow 2C_2H_5ONa + H_2$ From the stoichiometry,$2 \ mol$ of ethanol produces $1 \ mol$ of $H_2$ gas. At $S.T.P.$,$1 \ mol$ of any gas occupies $22400 \ mL$. Therefore,$22400 \ mL$ of $H_2$ is produced by $2 	imes 46 \ g$ of ethanol. $280 \ mL$ of $H_2$ is produced by: $\frac{2 	imes 46 	imes 280}{22400} \ g$ $= \frac{92 	imes 280}{22400} \ g$ $= \frac{92}{80} \ g = 1.15 \ g$. Thus,the correct option is $C$.

How many grams of ethanol are required to obtain $280 \ mL$ of dihydrogen gas at $S.T.P.$ by the reaction of $C_2H_5OH$ with $Na$ metal? (Molar mass of ethanol = $46 \ g/mol$)

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