The weight of calcium oxide formed by burning | vedclass

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(C) The balanced chemical equation for the reaction is: $2Ca + O_2 \rightarrow 2CaO$ Step $1$: Calculate the moles of $Ca$ used. $Moles \ of \ Ca = \f

Vedclass · Accepted Answer

$28$

Vedclass · Answer

(C) The balanced chemical equation for the reaction is: $2Ca + O_2 ightarrow 2CaO$ Step $1$: Calculate the moles of $Ca$ used. $Moles \ of \ Ca = \frac{	ext{Given mass}}{	ext{Molar mass}} = \frac{20 \ g}{40 \ g/mol} = 0.5 \ mol$ Step $2$: Use stoichiometry to find the moles of $CaO$ produced. From the equation,$2 \ mol$ of $Ca$ produces $2 \ mol$ of $CaO$,which means $1 \ mol$ of $Ca$ produces $1 \ mol$ of $CaO$. Therefore,$0.5 \ mol$ of $Ca$ will produce $0.5 \ mol$ of $CaO$. Step $3$: Calculate the mass of $CaO$. $Mass \ of \ CaO = 	ext{Moles} 	imes 	ext{Molar mass} = 0.5 \ mol 	imes 56 \ g/mol = 28 \ g$ Thus,the weight of calcium oxide formed is $28 \ g$.

The weight of calcium oxide formed by burning $20 \ g$ of calcium in excess oxygen is $.... \ g$

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