Ethanol is a fuel produced from plant products by fermentation. It has a density of $789 \mathrm{g} {\mathrm{dm}}^{-3}$ and its enthalpy of combustion is $-1367 \mathrm{kJ} {\mathrm{mol}}^{-1}$. Calculate the specific energy for ethanol. (Give the value approximated to a single decimal place)

Ethanol is a fuel produced from plant products by fermentation. It has a density of $789 \mathrm{g} {\mathrm{dm}}^{-3}$ and its enthalpy of combustion is $-1367 \mathrm{kJ} {\mathrm{mol}}^{-1}$. Write a balanced equation for the combustion of ethanol and state the amount, in $\mathrm{mol}$, of carbon dioxide produced per mole of ethanol burned.

Ethanol is a fuel produced from plant products by fermentation. It has a density of $789 \mathrm{g} {\mathrm{dm}}^{-3}$ and its enthalpy of combustion is $-1367 \mathrm{kJ} {\mathrm{mol}}^{-1}$. Explain why this method is still considered "green" chemistry even though it produces carbon dioxide in the combustion reaction.

Write balanced chemical equation, and predict products for the following process:

The cracking of ${\mathrm{C}}_{12}{\mathrm{H}}_{26}$ into two ethene molecules and an alkane.

Write balanced chemical equation, and predict products for the following process:

The reaction of char, $\mathrm{C}$, with steam to produce carbon monoxide and hydrogen gas.

Write balanced chemical equation, and predict products for the following process:

The production of methane from synthesis gas, $\mathrm{CO}$ and ${\mathrm{H}}_2$.

Write a balanced chemical equation, and predict products for the following process:

Catalytic reforming of heptane into methylbenzene.

Write balanced chemical equation, and predict products for the following process:

Liquefaction of synthesis gas, $\mathrm{CO}$ and ${\mathrm{H}}_2$ to produce liquid heptane.

Calculate the mass of carbon dioxide produced per gram of the ethanol burned. Give the value approximated to two decimal places.