Question

The hydrogenation of unsaturated hydrocarbons is


an important industrial process. Precious metals,


such as platinum and palladium, can greatly


increase the rate of this reaction. During this


process, the gaseous reactants are pumped


across a layer of metal powder. An example of this


process is shown below.


Describe how the metal probably increases the


reaction rate, identify whether this is an example


of homogeneous or heterogeneous catalysis, and


explain how you know.

Answer 1

Answer:

The metal catalyst in catalytic hydrogeation process increases the rate of reaction by lowering the activation energy of the reaction, by allowing the reaction take place at a much lower temperature than it would have without the metl ctalyst.

This catalysis is regarded as heterogeneous or surface catalysis.

Explanation:

The hydrogen is first bonded to the metallic powder as the initial step of the reaction.

Answer 2

Answer:

The metal probably increases reaction rate by either holding reactant molecules in the correct orientation to react or by weakening or breaking bonds in reactant molecules to make them more reactive.

This is an example of heterogeneous catalysis.

It is heterogeneous catalysis because the catalyst is a solid and the reactants are gases. In heterogeneous catalysis, the catalyst is in a different phase than the reactants.

Explanation: (edge explanation)