$$ \ce{C2H4(g) + H2(g) ->[platinum] C2H6(g)} $$

\(\ce{C2H4(g)}\) is reduced by \(\ce{H2(g)}\) in the presence of a solid platinum catalyst, as represented by the equation above. Factors that could affect the rate of the reaction include which of the following?

1. Changes in the partial pressure of \(\ce{H2(g)}\)
2. Changes in the particle size of the platinum catalyst
3. Changes in the temperature of the reaction system

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All of the factors listed would affect the rate of the reaction.

Changes in the partial pressure of any of the species would result in a change due to Le Chatlier's principle. This is because an increase in the number of reactant gas molecules increases the chance that a collision between reaction molecules occurs.

Similarly, changes in the catalyst size would affect the chance that the reactants have a suitable area to collide and react.

Temperature changes the speed of gas molecules, which also affects the chance that gas molecules collide with the correct amount of energy.