Effect of Temperature on Reaction Rates & the Concept of Activation Energy (CIE A Level Chemistry)

Fig. 1.1 below shows, for a given temperature T, a Boltzmann distribution of the kinetic energy of the molecules of a mixture of two gases that will react together.

The activation energy for the reaction, E_a, is marked.

Fig. 1.1

On Fig. 1.1 above,

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Explain the meaning of the term activation energy.

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Two reactions involving aqueous NaOH are given below.

The reagents in reaction 1 must be heated together for some time for the reaction to occur.
Whereas, reaction 2 is almost instantaneous at room temperature.

Suggest brief explanations why the rates of these two reactions are very different.

Ammonia can be produced by the reaction of nitrogen and hydrogen.

N₂ (g) + 3H₂ (g)  2NH₃ (g)          ΔH = -92 kJ mol^-1

The reaction can be catalysed and the activation energy for this catalysed reaction is +109 kJ mol^-1

Complete the reaction pathway diagram in Fig. 2.1 for the uncatalysed and the catalysed reaction between nitrogen and hydrogen.

You should label the following:

• products
• the enthalpy change of reaction, ΔH
• the activation energy of the forward, uncatalysed reaction, E_a
• the activation energy of the forward, catalysed reaction, E_c

Fig. 2.1

Calculate the value of the activation energy of the catalysed decomposition of ammonia into nitrogen and hydrogen.

Show your working.

activation energy .............................................. kJ mol^-1

Catalysts, such as iron used in the production of ammonia, increase the rate of reaction.

Explain why. Use a labelled Boltzmann distribution to explain your answer.

Platinum is used as a catalyst in catalytic converters which are fitted to vehicle exhaust systems to remove nitrogen oxide from the exhaust gases.

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In any chemical reaction, the particles will all be moving in different directions, at different speeds and with different amounts of energy. Maxwell-Boltzmann distributions show the distribution of energy amongst particles within a chemical reaction. 

Fig. 3.1 below shows the Maxwell-Boltzmann distribution in a sample of a gas at a fixed temperature, T₁. 

Fig. 3.1

State why a Maxwell-Boltzmann distribution curve always starts at the origin and what the area under the curve represents. 

Some changes were made individually to the experiment completed in part (a).

Consider your Maxwell-Boltzmann distribution curve from part (a). For each of the changes in parts (i), (ii) and (iii) below, state and explain the effect that the change would have on:

• The area under the curve
• The value of the most probably energy of the molecules (E_mp)
• The proportion of molecules with energy greater than or equal to E_a

A Maxwell-Boltzmann distribution curve is shown below in Fig 1.1 

Fig 1.1

For the changes detailed in part (i) and (ii) state and explain the effect the change would have on:

• The area under the curve 
• The value of the most probable energy of the molecules, E_mp
• The proportion of molecules with greater than or equal to E_a 

A chemist performed a reaction at three different temperatures, 100 K, 300 K and 700 K as shown by the Maxwell-Boltzmann distribution graph in Fig 1.2.

Fig 1.2

Hydrogen will react with chlorine to form the hydrogen halide, hydrogen chloride, a colourless gas.

H₂ (g) + Cl₂ (g) → 2HCl (g)

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