In which of the following beakers will a reaction occur? I: A beaker containing 1.0 M...
In which of the following beakers will a reaction occur?
I: A beaker containing 1.0 M HBr and Cl2(g)
II: A beaker containing 1.0 M HBr and Ag(s)
The answer is only I please explain why it is correct and how to solve
Homework Answers
This reactivity trend can be explained according to the reactivity series of metals and halogens.
In reactivity series of metals Ag (silver) lies below of hydrogen and the general rule is that a metal can dispalce any metal which is lower than that in thi series . Ag being at a lower position than hydrogen can't displace hydrogen from HBr.
The same rule applies for halogen series also. While fluorine being most reactive , chlorine is next to it, after which Bromine comes. Chlorine is at a higher position than bromine so it can easily dispace Br- from HBr to produce HCl.
So reaction 1 only happens .
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