Answer:
Explanation:
Chemical reactions follow a path: reactants increase their chemical energies, form activated complexes (transition compounds) until reaching the activation energy, from which the final products are formed.
Catalysts are substances that can change the path of the reactions by lowering the activation energy (first statement is true) and, consequently, speeding up the reaction (third statement is true).
The activation energy is the minimum amount of energy required for the reactants to form the activated complex. So, catalysts, by providing a new path, where the activation energy is lower, manage to incrase the rate of the reaction.
But catalysts, although intervene in the reaction by modifying the way the reactants will react, do not form part of the reactants nor products, so they are not consumed by the overall reaction (second statement is false).
Answer:
True:
Catalysts speed up chemical reactions
Catalysts lower activation energy
False:
Catalysts are consumed by the overall reaction
Explanation:
A catalyst is a substance that provides an alternate pathway of lower activation energy for the reaction to proceed. By lowering the activation energy, a catalyst speeds up the chemical reaction but s not consumed overall.
