Heat of solution for sulfuric acid in water

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To calculate the enthalpy of solution for sulfuric acid at 30°C for concentrations of 0.2, 0.5, and 1 mol/kg, an enthalpy-concentration diagram is suggested, though the user struggles to interpret it. The discussion highlights the need for specific data regarding the concentrations of sulfuric acid and water to perform the calculations accurately. The user seeks assistance in understanding the diagram and the necessary data for their theoretical calculations. They aim to compare the theoretical enthalpy values with their experimental results. Clarification on the diagram and data interpretation is essential for accurate calculations.
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Homework Statement



How can I calculate the enthalpy of solution for sulfuric acid at 30°C/68°F, for 0,2;0,5;1 mol/kg?

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The Attempt at a Solution


I tried using a enthalpy-concentration diagram, but I cannot read it. I would apreciate if anyone could help me!
 
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what is this diagram you have? what data are you provided with?
 
This one: http://docs.google.com/gview?a=v&q=cache:sexRAoFSlI4J:www.norfalco.com/documents/NorFalco_H2SO4Property07.pdf+calculate+enthalpy+sulfuric+acid&hl=en&gl=br

The only data I got is the concentration of the solution H2SO4 and water. I needed to find the theoretical enthalpy of solution for this reaction, to compare with the results I got from the experiment.
 
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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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