The discussion revolves around the concept of activation energy and its effect on the rate of chemical reactions, as well as the differences between geometric isomers in alkenes and alkanes.
Some participants have provided insights into the relationship between activation energy and reaction rates, with a focus on how catalysts may lower activation energy. There is an ongoing exploration of additional methods to increase reaction rates, and participants are questioning and clarifying their understanding of these concepts.
Participants express uncertainty about the definitions and implications of catalysts and activation energy, indicating a need for further clarification on these topics.
joejo said:thx that clears things up a bit...As for increasing the rate of chemical reaction are there any more ways or just those...
WhirlwindMonk said:Temperature and in some cases, the concentration of the reactants, depending on the order of the reaction (if you are unsure of what I'm talking about, just ignore it).
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sorry, i didn't read your whole post. And i don't think catalysts speed up the reaction, they simply allow it to occur at a lower energy state by lowering the activation energy.
bross7 said:Lowering the activation energy is speeding up the reaction. Think of it in terms of a linear distance. If I am 5 miles from a store one day and 3 miles the next day, when will I get there faster?