write down an example compound for all the oxidation states of nitrogen, including hydrides, halides, oxyacids and oxides
give several examples of nitrogen-containing explosives and explain how they function
give a molecular interpretation/rationalization for the exothermicity of combustion reactions leading to CO2, H2O and N2
distinguish between (explosive) decomposition and combustion reactions
list the oxides and oxyacids of nitrogen and calculate the oxidation number of nitrogen
distinguish primary and secondary pollutants
write down the key reactions for the nitrogen atmospheric cycle, and use them to explain the generation of secondary pollutants nitrogen dioxide and ozone
describe the mechanism of atmospheric generation of nitric acid through the nitrate radical, and explain why this becomes significant at dusk and is affected by humidity and pollution
use the Second Law to determine whether a reaction will be spontaneous at high or low temperatures (or neither or both)
explain chemical equilibrium as a reaction mixture whose composition is unchanging in time, and relate this to the kinetic picture of equal rates of formation and decomposition of reactants and products
define the equilibrium constant, and write it down for an arbitrary gas phase reaction
calculate the value of the equilibrium constant for a reverse reaction from its value for a forward reaction, and if the stoichiometry is changed
calculate the equilibrium constant for a reaction obtained by combining two other reactions
calculate equilibrium compositions from starting compositions and the equilibrium constant for a simple gas phase reaction
calculate the equilibrium composition for a chemical reaction from its equilibrium constant and mass balance information
use appropriate aproximations for simplifying such calculations
define the reaction quotient and use it to predict the direction of change in a reaction as it approaches equilibrium, or if it is perturbed from equilibrium.
use the enthalpy of reaction to predict how the equilibrium constant changes with temperature
explain that catalysts change the pathway and rate of reaction but not the position of equilibrium
explain that entropy depends on concentration, but enthalpy can be treated as independent of concentration
explain the reasons for the conditions used in the Haber Process, and apply the same reasoning to the optimization of other chemical processes, such as smelting
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