What are the key factors to consider in the preparation of bromine gas?

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Key factors to consider in the preparation of bromine gas include understanding the nature of the reaction, which involves oxidation and reduction processes, as well as the bonding types present. The reaction is exothermic, and analyzing the entropy changes is crucial for predicting the spontaneity of the reaction. It is also important to assess the number of particles involved before and after the reaction, including their states and complexities. Additionally, measuring the rate of reaction and determining any changes in pH during the process are essential components of the lab work. Gathering detailed information from textbooks and reliable online sources will aid in successfully completing the assignment.
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Homework Statement



Ok hi. I have this reaction for a lab due in about 2 weeks. It is on the preperation of bromine gas. The exact reaction was assigned (which is why i didn't choose a less-complex method, such as 2KBr + Cl2 --> 2KCl + Br2). My problem is that i need information (ie. internet websites, textbooks) becasue i need to have information such as:

- nature of reaction (atomic/molecular)
- bonding (intermolecular/intramolecular)
- energy (endo/exothermic)
- entropy (chaos)
- number of particles before and after, state of particle, complexity of part
- rate of reaction (actually, that's what my lab will be about)
- acidic/basic/redox

Homework Equations


2KBr + MnO2 + 2H2SO4 --> K2SO4 + MnSO4 + 2H2O + Br2 (gas)


The Attempt at a Solution



I have looked through numerous textbooks at the public library and websites and haven't found any information on this reaction. If anyone has informaiton on this reaction, that would be very helpful.
 
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oh yeah, and since this is my first time ever participating in this forum, please tell me if I'm missing anything
 
You have a good start already. In what oxidation state are bromide and manganese oxide. How about manganese sulfate and bromine gas? Is anything being oxidized or reduced? Can you calculate the enthalpy of the reaction? Will the pH change during the reaction?

You probably know these answers already from your coursework. How will you measure the rate of reaction in the lab?
 
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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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