Glossary (NEW)

The number of particles in one mole of particles (see mole).  Measured to be
NA = 6.0221×10-23

[Latexpage]

This is a named reaction type.  Generally, a combustion reaction for a certain compound involves the complete combustion in oxygen of one mole of said compound to it's fully oxidized products.  If the compound in question is a carbohydrate, the products are carbon dioxide and water.  If there are other elements in the compound, the products would have to include the fully oxidized form of those elements.  For example, the combustion reaction for ethane, C2H6 is
C2H6 + 3.5 O2  2 CO2 + 3 [latex]H_2O[/latex].
Note: the coefficient for the ethane MUST be 1 for it to be called the combustion reaction.  The following balanced equation shows the same chemical process but is not the defined combustion equation.
2 C2H6 + 7 O2  4 CO2 + 6 H2O.
The combustion reaction for ethylamine has to have NO2 as a product in addition to carbon dioxide and water.
CH3NH2 + 3.25 O2  CO2 + NO2 + 2.5 H2O

The Extended Fraction formalism is a means of performing conversions of units and/or dimensions by expanding all the individual fractions in a problem to full explicit forms and then putting them into a single fractional form in a way that ensures the proper units cancel to leave the desired units of the answer. Thus, implied fractions such as molar mass (g/mol), percent by mass (g/100g), concentrations (mol/L or mol/kg) mole fractions (mole/total mole) and even stoichiometric factors can be encorporated into a mathematical calculation in a single large fraction where each smaller fraction is divided from it's neighbour by vertical lines in the larger fraction. Example, to convert from g of hydrogen to moles of hydrogen, we use the molar mass as a conversion factor. Note that we have written the molar mass conversion factor seemingly inverted here but that is what is required to cancel the units "g H" to leave the desired units "mol H". This method is first discussed in the course notes here.

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