What is the benefit of using a shortcut in a reaction between two chemicals? A shortcut would ensure a safer reaction. A shortcut may provide a faster reaction. A reaction with a shortcut would yield more chemical output. A reaction with a shortcut would require less chemical input.

A shortcut may provide a faster reaction

Explanation:

Chemical reactions occur in a particular manner and speed if allowed to occur normally. However, shortcuts can be used for the essence of making the reaction proceed much faster than it naturally would. Catalysts are the substances used to provide these shortcuts.

A catalyst is a substance that increases the rate at which a chemical reaction occurs without being chemically used up in the reaction. A catalyst speedens up the chemical reaction by decreasing the activation energy. The activation energy is that energy needed for a chemical reaction to kick start. The higher the activation energy, the slower the reaction proceeds.

A catalyst, thus, creates a shortcut by lowering the activation energy of the chemical reaction, allowing it to proceed faster than when a catalyst is not used.

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it provides an alternative energy pathway for the reaction to proceed.

a catalyst is a substance that speeds up the rate of a chemical reaction but is not consumed during the course of the reaction.

catalysts increase the rate of reaction without being used up. they do this by lowering the activation energy needed. with a catalyst, more collisions result in a reaction, so the rate of reaction increases. different reactions need different catalysts.

a catalyst works by providing an alternative reaction pathway to the reaction product. the rate of the reaction is increased as this alternative route has a lower activation energy than the reaction route not mediated by the catalyst.