Describe how the metal probably increases the reaction rate, identify whether this an example of homogeneous or heterogeneous catalysts, and explain how you know.

Explanation:

The metal probably helps to speed up the reaction rate a/c to collision theory, reactant molecules must collide with a reasonable direction by either weakening bonds in reactant molecules to make them extra reactive or by attaching reactant molecules in the exact direction to react.

This is known as an example of heterogeneous catalysis because the catalyst is solid and the reactants are liquid or gases mixture. In this catalysis, the catalyst is present in a different phase compare to the reactants.

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.