Write Down the Chemical Formulae for the Combustion of the Alkanes

Question

Examlex · Accepted Answer

The Answer is The oxidation process is shown below

\begin{array} { l l l l } \hline n & ext { name } & ext { formula } & ext { combustion reaction } \\hline 2 & ext { ethane } & \mathrm { C } _ { 2 } \mathrm { H } _ { 6 } & 2 \mathrm { C } _ { 2 } \mathrm { H } _ { 6 } + 7 \mathrm { O } _ { 2 } ightarrow 4 \mathrm { CO } _ { 2 } + 6 \mathrm { H } _ { 2 } \mathrm { O } \3 & ext { propane } & \mathrm { C } _ { 3 } \mathrm { H } _ { 8 } & \mathrm { C } _ { 3 } \mathrm { H } _ { 8 } + 5 \mathrm { O } _ { 2 } ightarrow 3 \mathrm { CO } _ { 2 } + 4 \mathrm { H } _ { 2 } \mathrm { O } \4 & ext { butane } & \mathrm { C } _ { 4 } \mathrm { H } _ { 10 } & 2 \mathrm { C } _ { 4 } \mathrm { H } _ { 10 } + 13 \mathrm { O } _ { 2 } ightarrow 8 \mathrm { CO } _ { 2 } + 10 \mathrm { H } _ { 2 } \mathrm { O } \5 & ext { pentane } & \mathrm { C } _ { 5 } \mathrm { H } _ { 12 } & \mathrm { C } _ { 5 } \mathrm { H } _ { 12 } + 8 \mathrm { O } _ { 2 } ightarrow 5 \mathrm { CO } _ { 2 } + 6 \mathrm { H } _ { 2 } \mathrm { O } \6 & ext { hexane } & \mathrm { C } _ { 6 } \mathrm { H } _ { 14 } & 2 \mathrm { C } _ { 6 } \mathrm { H } _ { 14 } + 19 \mathrm { O } _ { 2 } ightarrow 12 \mathrm { CO } _ { 2 } + 14 \mathrm { H } _ { 2 } \mathrm { O } \7 & ext { heptane } & \mathrm { C } _ { 7 } \mathrm { H } _ { 16 } & \mathrm { C } _ { 7 } \mathrm { H } _ { 16 } + 11 \mathrm { O } _ { 2 } ightarrow 7 \mathrm { CO } _ { 2 } + 8 \mathrm { H } _ { 2 } \mathrm { O } \8 & ext { octane } & \mathrm { C } _ { 8 } \mathrm { H } _ { 18 } & 2 \mathrm { C } _ { 8 } \mathrm { H } _ { 18 } + 25 \mathrm { O } _ { 2 } ightarrow 16 \mathrm { CO } _ { 2 } + 18 \mathrm { H } _ { 2 } \mathrm { O } \\hline\end{array}

The number of moles of

\mathrm { CO } _ { 2 }

produced per mole of alkane is clearly shown. The molecular mass of the alkane is shown below. The molecular mass

( M )

of

\mathrm { CO } _ { 2 } ( 44 \mathrm {~g} / \mathrm { mol } )

can be used to determine the relative mass of

\mathrm { CO } _ { 2 }

produced per unit mass of alkane. The heat of combustion is given in Table

3.2

and the amount of

\mathrm { CO } _ { 2 }

per

\mathrm { MJ }

heat is found.

\begin{array}{llllll}\hline n & \begin{array}{l}R=( ext { moles } \\left.\mathrm{CO}_{2} ight) /( ext { moles } \ ext { alkane) }\end{array} & \begin{array}{l}M \ ext { (alkane) }\end{array} & \begin{array}{l}R imes 44 / M= \\left(\mathrm{kg} \mathrm{CO}_{2} ight) /(\mathrm{kg} ext { alkane) }\end{array} & \begin{array}{l} ext { heat of } \ ext { combustion } \\mathrm{MJ} / \mathrm{kg}\end{array} & \mathrm{kg}\left(\mathrm{CO}_{2} ight) / \mathrm{MJ} \\hline 2 & 2 & 30 & 2.93 & 51.9 & 0.0565 \3 & 3 & 44 & 3.00 & 50.3 & 0.0596 \4 & 4 & 58 & 3.03 & 49.5 & 0.0612 \5 & 5 & 72 & 3.06 & 48.7 & 0.0628 \6 & 6 & 86 & 3.07 & 48.1 & 0.0638 \7 & 7 & 100 & 3.08 & 48.1 & 0.0640 \8 & 8 & 114 & 3.09 & 46.8 & 0.0660 \\hline\end{array}

Write Down the Chemical Formulae for the Combustion of the Alkanes

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Write Down the Chemical Formulae for the Combustion of the Alkanes

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