SSCE VCE Chemistry Extent of Chemical Reactions: Carbon monoxide and hydrogen can

Question

Carbon monoxide and hydrogen can be produced from the reaction of methane with steam according to the equation
$$\text{CH}_4(g) + \text{H}_2\text{O}(g) \rightleftharpoons \text{CO}(g) + 3\text{H}_2(g); \Delta H = +206 \text{ kJ mol}^{-1}$$

Some methane and steam are placed in a closed container and allowed to react at a fixed temperature. The following graph shows the change in concentration of methane and carbon monoxide as the reaction progresses.

1. On the graph above, draw a line to show the change in concentration of hydrogen gas as the reaction progresses. Label this line.
2. On the graph above, draw a line to show the formation of carbon monoxide would differ over time in the presence of a catalyst. Label this line.

Great care must be taken when handling carbon monoxide as it is a highly poisonous gas. Even at low concentrations it competes very successfully with oxygen for haemoglobin, the oxygen carrier in the blood.

The reactions can be written as
$$\text{haemoglobin} + \text{oxygen} \rightleftharpoons \text{oxyhaemoglobin}; \text{K}_1$$
$$\text{haemoglobin} + \text{carbon monoxide} \rightleftharpoons \text{carbon monoxide-haemoglobin}; \text{K}_2$$
What does the above information indicate about the magnitude of the equilibrium constant $K_1$ compared with the magnitude of the equilibrium constant $K_2$?

The rates of chemical reactions may be explained using the collision theory model. Indicate whether the following statements about the rates of chemical reactions and the collision theory model are true or false by placing ticks in the appropriate boxes.

1. Endothermic reactions are always slower than exothermic reactions.
2. All particles have the same kinetic energy at a fixed temperature.
3. Reactant particles collide.
4. The rate of reaction at a constant temperature increases when the concentration increases.
5. Temperature increases the fraction of collisions with energy.

On the graph above, draw a line to show the change in concentration of hydrogen gas as the reaction progresses. Label this line.

On the graph above, draw a line to show the formation of carbon monoxide would differ over time in the presence of a catalyst. Label this line.

What does the above information indicate about the magnitude of the equilibrium constant K₁ compared with the magnitude of the equilibrium constant K₂?

Endothermic reactions are always slower than exothermic reactions.

All particles have the same kinetic energy at a fixed temperature.

Reactant particles collide.

The rate of reaction at a constant temperature increases when the concentration increases.

Temperature increases the fraction of collisions with energy.

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