Sherlock Potter
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Is this reaction endothermic?

CaO +HCl -> CaCl2 + H2O


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Pigster
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No, and it isn't balanced either.
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Sherlock Potter
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(Original post by Pigster)
No, and it isn't balanced either.
Ooops thanks


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Pride
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It's exothermic, which means it gives off heat. Endothermic reactions take in heat from the surroundings.
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Kallisto
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Whenever reagents start to react, energy is released, so exothermic. This energy is giving off by heat. Exothermic energy is exhausted when the reaction is over. The energy which is required to cause an reaction is the activation energy. This energy has to spend (in form of heat in surroundings for instance), that is endothermic.

In short your chemical equation is exothermic.
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Sherlock Potter
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Thanks everyone very helpful answers


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Pigster
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(Original post by Kallisto)
Whenever reagents start to react, energy is released, so exothermic. This energy is giving off by heat. Exothermic energy is exhausted when the reaction is over. The energy which is required to cause an reaction is the activation energy. This energy has to spend (in form of heat in surroundings for instance), that is endothermic.

In short your chemical equation is exothermic.
It is worth pointing out that at least some of this makes sense.

If you don't know which bits, you're welcome to enquire.
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Kallisto
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I thought that a reaction consists of an endergonic and exergonic reaction processes in general. In endergonic energy is taken to enable a reaction between reagents. When the reaction begins, energy is giving off during the reaction process. Sounds plausible, is that not right?
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Pigster
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If you changed "energy is giving off during the reaction process" to "energy is giving off during that/those stage/s of the reaction process", then I'd be happier.

In more GCSE/AS language, "Energy is needed to break bond and energy is released making bonds. If more energy is released than taken in, the reaction is exothermic."

Or at A2, when students do Born Haber cycles... they are taught a load of boswellox and are given the impression that gaseous atoms and ions are created in a certain order and so forth. But still it boils down to ions form (endo - usually) and lattices build up (exo).
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Kallisto
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(Original post by Pigster)
If you changed "energy is giving off during the reaction process" to "energy is giving off during that/those stage/s of the reaction process", then I'd be happier.

In more GCSE/AS language, "Energy is needed to break bond and energy is released making bonds. If more energy is released than taken in, the reaction is exothermic."
That is veeery precisely, but you are right. I didn't have consider it from this view so far. Thanks for giving me a new view.

So when CaO and HCl are breaking to the ion parts, energy is taken by surroounding (endothermic reaction). And when these ions begin to react to products, energy is released at every stage of the reaction, so at every single moment of the reaction (exothermic reaction), right?
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