a. Energy conversion based on hydrocarbon fuel combustion leads to the formation ofpollutants. In internal combustion (IC) engine applications, a catalytic converter isan exhaust emission control device that converts toxic gases and pollutants in exhaustgas from an IC engine into less-toxic pollutants by catalysing a reduction/oxidationreaction. List the main categories of these pollutants and briefly explain the conversiontaking place in a catalytic converter.b. Ammonia (NH3) is a zero-carbon fuel that can be used in combustion applications, butNH3 combustion also leads to harmful substances. List the main substances and (inone sentence) state their harmful impacts.c. The decomposition of nitrogen dioxide is given by 2??2 (?→) 2?? + ?2. In an experiment,the reaction rate constant has been measured at two temperatures, obtaining thefollowing values:? (K) / ?(cm3/mol/s)592 / 500627 / 1810(i) Find the decomposition rate (in SI unit) of NO2 at 592 K if its concentration is 4.0mol/cm3(ii) Find the activation energy of this decomposition reaction, assuming that theArrhenius equation can be used to describe the dependence of the rate constant ontemperature (taking the molar gas constant ? = 8.314 J/mol/K).

a. Energy conversion based on hydrocarbon fuel combustion leads to the formation of
pollutants. In internal combustion (IC) engine applications, a catalytic converter is
an exhaust emission control device that converts toxic gases and pollutants in exhaust
gas from an IC engine into less-toxic pollutants by catalysing a reduction/oxidation
reaction. List the main categories of these pollutants and briefly explain the conversion
taking place in a catalytic converter.

b. Ammonia (NH3) is a zero-carbon fuel that can be used in combustion applications, but
NH3 combustion also leads to harmful substances. List the main substances and (in
one sentence) state their harmful impacts.

c. The decomposition of nitrogen dioxide is given by 2??2 (?→) 2?? + ?2. In an experiment,
the reaction rate constant has been measured at two temperatures, obtaining the
following values:
? (K) / ?(cm3/mol/s)
592 / 500
627 / 1810

(i) Find the decomposition rate (in SI unit) of NO2 at 592 K if its concentration is 4.0
mol/cm3

(ii) Find the activation energy of this decomposition reaction, assuming that the
Arrhenius equation can be used to describe the dependence of the rate constant on
temperature (taking the molar gas constant ? = 8.314 J/mol/K).