Instructions: For each of the following reactions, consult the "Standard Reduction Potentials" AP handout to see if the reaction will occur. If the reaction does occur, write the unbalanced net ionic equation; otherwise, write "No Reaction."
a) Solid beryllium metal is added to a solution of iron (ii) chloride.
b) A bar of solid tin is added to an aluminum chlorate solution.
c) A lead pipe is exposed to a sodium acetate solution.
d) Copper wire is dropped into a silver nitrate solution.
I'd be thankful if anyone helps me out with these problems. Tell me how to get the right answer, if you don't mind.
Thank you in advance!
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Alright ill try to explain this. You should have a list that says x elements in order, we'll refer to this as A, B, C and D.
A is most reactive and D is least.
Now the SOLID metal will try to switch with the solution ONLY if It is closer to A than the metal in solution B. ie:
Solid B is dropped into a solution of C nitrate(doesnt matter) Now since B is MORE reactive, it's going to try to switch places with the nitrate, and so a reaction occurs
B + CNO3 > C + BNO3
I hope this makes sense sort of