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Determine the value of the rate constant for the reaction Br2 + H2 = 2HBr if [Br2] = 0.15 M, [H2] = 0.2 and the rate of the reaction is 0.005 M s^-1 at 298 K
I don't want to know the different equations for it ... I want to know the difference between those reaction types. What does a reaction need to be classified as 1st, 2nd, or 3rd order? What are the differences?
What is Rate Law of the reaction below?$$\ce{4 HBr + O2 -> 2 H2O + 2 Br2}$$
How do we approach finding the rate law of reaction? Can this be found out only through experiments?
this exercise did not came out of nothing ... there must have been similar exercises or sth during your lectures that prepared you for this. if not, then google yields tons of information on that problem.
It's really the relativistic effects that foul everything up.
Once you get past copper or so, you just about can't avoid dealing with them.
ECPs are great to a point, but AFAIK they munge up a lot of methods
scalar relativistics like DKH and ZORA/IORA are okay for energies and geometries, but I think fail in weird ways for the subtler things like SOC, ZFS, etc.
Is it because we're past the newly-graduated phase, but don't have a critical mass of membership to result in the small fraction of engaged members being more than a handful of people?
Is okay, I'm working on some other stuff alongside.
At least with only a single metal and a ~normal organic ligand environment, I would think you weren't/aren't facing any antiferromagnetic behavior or anything.
the latter, yes. but the heteroaromatic system seems to need multireference treatment ... I need to find out more about this. (T1 diagnostic and the new FOD analysis told sth like that)
I'll be back in about ~30-60 mins ... if you are still there, we can continue to talk about it
What is Rate Law of the reaction below?$$\ce{4 HBr + O2 -> 2 H2O + 2 Br2}$$
How do we approach finding the rate law of reaction? Can this be found out only through experiments?
The Periodic Table
The Periodic Table