Sergey Bylikin, Gary Horner and, Brian Murphy Solutions for Chapter: Energy, Exercise 2: Questions

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.

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

Calculate the mass of carbon dioxide produced per gram of $2,2,4-$trimethylpentane burned. Give the value approximated to two decimal places.

The enthalpies of combustion of the three fuels are:

ethanol $-1367 \mathrm{kJ} {\mathrm{mol}}^{-1}$; methane $-891 \mathrm{kJ} {\mathrm{mol}}^{-1}$; $2,2,4$-trimethylpentane $-5460 \mathrm{kJ} {\mathrm{mol}}^{-1}$

Calculate the energy released in burning $1 \mathrm{g}$ (the specific energy) of each fuel.

The 

Discuss the advantages and disadvantages of each fuel and the problems faced by society in using "green" fuels.