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(A) The chemical equation for the complete combustion of $n$-butane $(C_4H_{10})$ is:$2C_4H_{10} + 13O_2 \rightarrow 8CO_2 + 10H_2O$First, calculate t

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$352$

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(A) The chemical equation for the complete combustion of $n$-butane $(C_4H_{10})$ is:$2C_4H_{10} + 13O_2 ightarrow 8CO_2 + 10H_2O$First, calculate the molar mass of $n$-butane $(C_4H_{10})$:$M(C_4H_{10}) = 4 	imes 12 + 10 	imes 1 = 48 + 10 = 58 \ g/mol$Calculate the number of moles of $n$-butane in $116 \ g$:$n = \frac{116 \ g}{58 \ g/mol} = 2 \ mol$From the balanced equation, $2 \ mol$ of $C_4H_{10}$ produces $8 \ mol$ of $CO_2$.Calculate the mass of $CO_2$ produced:Molar mass of $CO_2 = 12 + 2 	imes 16 = 44 \ g/mol$Mass of $CO_2 = 8 \ mol 	imes 44 \ g/mol = 352 \ g$.

The amount of carbon dioxide evolved upon complete combustion of $116 \ g$ of $n$-butane is
(Given : atomic mass in amu $H = 1, C = 12$ and $O = 16$) (in $g$)

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The amount of carbon dioxide evolved upon complete combustion of $116 \ g$ of $n$-butane is(Given : atomic mass in amu $H = 1, C = 12$ and $O = 16$) (in $g$)