Don't know how to do this stoichiometric problem with 4 questions.

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The discussion revolves around a stoichiometric problem involving copper compounds. The user has successfully answered the first three questions but is confused about the role of CuO, questioning its relevance compared to Cu(OH)2. It is clarified that CuO is a product of the decomposition of copper hydroxide, which can be represented as Cu(OH)2 decomposing into CuO and water. The conversation emphasizes that while copper hydroxide can decompose, copper oxide does not react with water. Understanding these chemical transformations is crucial for solving the stoichiometric problem effectively.
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Homework Statement



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Homework Equations



n/a

The Attempt at a Solution



I got the first 3 answers. But I don't know what this is asking for. What is CuO. Where did that come from. Is \n't it supposed to be Cu(OH)2?
 

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CuO + H_2O \rightarrow Cu(OH)_2
It is just hydrated form, nothing to worry about.
 
I would put it as

Cu(OH)2 -> CuO + H2O

copper hydroxide easily decomposes, but copper oxide doesn't react with water.
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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