What is the amount of water formed by combust | vedclass

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(C) The balanced chemical equation for the combustion of methane is: $CH_4 + 2 O_2 \rightarrow CO_2 + 2 H_2 O$Calculate the moles of methane $(CH_4)$:

Vedclass · Accepted Answer

$3.6$

Vedclass · Answer

(C) The balanced chemical equation for the combustion of methane is: $CH_4 + 2 O_2 ightarrow CO_2 + 2 H_2 O$Calculate the moles of methane $(CH_4)$: Molar mass of $CH_4 = 12 + (4 	imes 1) = 16 \ g/mol$. Moles $= \frac{1.6 \ g}{16 \ g/mol} = 0.1 \ mol$.From the stoichiometry of the reaction,$1 \ mol$ of $CH_4$ produces $2 \ mol$ of $H_2 O$. Therefore,$0.1 \ mol$ of $CH_4$ will produce $0.1 	imes 2 = 0.2 \ mol$ of $H_2 O$.Calculate the mass of water $(H_2 O)$: Molar mass of $H_2 O = (2 	imes 1) + 16 = 18 \ g/mol$. Mass $= 0.2 \ mol 	imes 18 \ g/mol = 3.6 \ g$.

What is the amount of water formed by combustion of $1.6 \ g$ methane (in $g$)?

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