Lawrie Ryan and Roger Norris Solutions for Chapter: Rates of Reaction, Exercise 14: EXAM-STYLE QUESTIONS

Shade an area on the graph to show the additional number of molecules capable of reacting because of the presence of a catalyst.

Draw a curve on your graph to show the Boltzmann distribution of molecular energies at a slightly higher temperature.

The Haber process is used in industry to convert nitrogen and hydrogen to ammonia. The formation of ammonia gas is exothermic. Sketch the enthalpy profile for the Haber process in absence of catalyst. 

The Haber process is used in industry to convert nitrogen and hydrogen to ammonia. The formation of ammonia gas is exothermic. Sketch the enthalpy profile for the Haber process in presence of a catalyst. 

The Haber process is used in industry to convert nitrogen and hydrogen to ammonia. The formation of ammonia gas is exothermic. Label the activation energy on the energy profile.

The activation energy for the uncatalysed decomposition of ammonia to its elements is ${+335 \mathrm{kJ} \mathrm{mol}}^{-1}$. Write the equation for this reaction including state symbols.

The activation energy for the uncatalysed decomposition of ammonia to its elements is ${+335 \mathrm{kJ} \mathrm{mol}}^{-1}$. The enthalpy of reaction for this decomposition is $+92 \mathrm{kJ} {\mathrm{mol}}^{-}$. Calculate the activation energy for the uncatalysed formation of ammonia from nitrogen and hydrogen.

The activation energy for the uncatalysed decomposition of ammonia to its elements is ${+335 \mathrm{kJ} \mathrm{mol}}^{-1}$. If tungsten is used as a catalyst, the activation energy changes. Explain how it will change.