A level Chemistry heterogeneous catalyst help!!

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medicnia20
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“Describe how a heterogeneous catalyst increases the rate of reaction [3marks]”

Can someone please write out a model answer for this question please, i know its pretty easy, I’m not sure why I’m finding it challenging, thanks!
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Sick0_M0de
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A heterogeneous catalyst is a catalyst that is in the same state as the reactants. Catalysts work by providing an alternative reaction pathway with a lower activation energy thus increasing the rate of reaction.
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kristenVigil
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I believe heterogeneous = different phase.
Something about reactant adsorb onto the surface of the catalyst.
Do you have access to this question's marking scheme? Try to formulate your answer base on that.
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scimus63
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not sure what the mark scheme says but if one reactants is adsorbed onto surface of the catalyst, the bonds in the reactants maybe broken and the new bonds with the catalyst are weak, so a second reactant can react with the one on the catalyst - this will have a reduced activation energy.

Both reactants can be adsorbed onto the catalyst surface and can "wander " freely over the surface where they can collide and react, they then leave the catalyst surface easily as bonds to the catalyst are weak.

One reactant can be absorbed onto the surface and be held in a particularly favourable geometry for the second or other reactants to reactant with it.

All of the above as someone else mentioned have lower activation energy, and since this is lower it will be faster to.

not sure if this helps much but its all I have got!
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gogrizz123
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(Original post by medicnia20)
“Describe how a heterogeneous catalyst increases the rate of reaction [3marks]”

Can someone please write out a model answer for this question please, i know its pretty easy, I’m not sure why I’m finding it challenging, thanks!
A catalyst that is not in the same state as the reactants, works by providing an alternative reaction pathway with less Ea, so more molecules have E>Ea, you get more successful collisions and as such a faster rate of reaction.
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