What is the Theoretical Heat of Hydration for Copper(II) Sulphate?

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The theoretical heat of hydration for anhydrous copper(II) sulfate is not readily available in common thermodynamic data sources, including the CRC Handbook. Users suggest calculating it from the standard heats of formation for both anhydrous copper(II) sulfate and its pentahydrate. The relevant reaction involves the hydration of CuSO4 with five water molecules. A key consideration in these calculations is determining the appropriate heat of formation value for water, whether as a gas or liquid. Accurate calculations require careful attention to these thermodynamic details.
nathaniell
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Hey poeple do any of you know what is the theoretical value for the heat of hydartion of copper

I need it to make some calculations in my lab
 
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Cupric sulfate? It comes in two flavors, anhydrous and as the pentahydrate.
 
Yes I want the heat of anhydrous copper(II) sulphate
 
Sorry, I misread your OP to mean heat of solution...

I have been having trouble finding thermodynamic data for anhydrous cupric sulfate as far as heat of hydration. I am only using the internet and my latest edition of the CRC (84th ed). Its not there.

You might find this in the library or you could calculate from the standard heats of formation for the anhydride and the pentahydrate. There are some tricks to the calculation...

The reaction would be:

CuSO4 + 5 H2O -----> CuSO4(5H2O)

You can easily find the standard heat of formation for the anhydride and the pentahydrate but what value should you use for the 5H2O? The heat of formation of the gas or the liquid?
 
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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