The masses of carbon dioxide and water (in g) | vedclass

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(B) The balanced chemical equation for the combustion of glucose is: $C_6H_{12}O_6 + 6O_2 \longrightarrow 6CO_2 + 6H_2O$ The molar mass of glucose $(C

Vedclass · Accepted Answer

$14.66, 6.0$

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(B) The balanced chemical equation for the combustion of glucose is: $C_6H_{12}O_6 + 6O_2 \longrightarrow 6CO_2 + 6H_2O$ The molar mass of glucose $(C_6H_{12}O_6)$ is $180 \ g/mol$. From the stoichiometry,$1 \ mol$ of glucose $(180 \ g)$ produces $6 \ mol$ of $CO_2$ $(6 	imes 44 = 264 \ g)$ and $6 \ mol$ of $H_2O$ $(6 	imes 18 = 108 \ g)$. For $10 \ g$ of glucose: Mass of $CO_2 = \frac{264 \ g}{180 \ g} 	imes 10 \ g = 14.66 \ g$. Mass of $H_2O = \frac{108 \ g}{180 \ g} 	imes 10 \ g = 6.0 \ g$.

The masses of carbon dioxide and water (in $g$) respectively formed during complete combustion of $10 \ g$ of glucose at $STP$ are

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