8 g of CH_4 is completely burnt in air. The | vedclass

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(C) The balanced chemical equation for the combustion of methane is: $CH_4(g) + 2O_2(g) 	o CO_2(g) + 2H_2O(l)$.The molar mass of $CH_4$ is $12 + (4 \

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(C) The balanced chemical equation for the combustion of methane is: $CH_4(g) + 2O_2(g) 	o CO_2(g) + 2H_2O(l)$.The molar mass of $CH_4$ is $12 + (4 	imes 1) = 16 \ g/mol$.The number of moles of $CH_4$ is calculated as: $n = \frac{	ext{mass}}{	ext{molar mass}} = \frac{8 \ g}{16 \ g/mol} = 0.5 \ mol$.According to the stoichiometry of the reaction,$1 \ mol$ of $CH_4$ produces $2 \ mol$ of $H_2O$.Therefore,$0.5 \ mol$ of $CH_4$ will produce $0.5 	imes 2 = 1 \ mol$ of $H_2O$.

$8 \ g$ of $CH_4$ is completely burnt in air. The number of moles of water produced are $.....$

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