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- Dec 25, 2015
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If somebody would please please please pretty please explain this to me, I would be so eternally grateful...
What I understand:
Zn(s) + HCl --> H2(g), which means that 1) H+ gets reduced and 2) the reaction is spontaneous. The question asks if a strip of Al(s) is placed in a beaker, will H2(g) evolve?
Then, we look at the table. We see that for Al(s) + Zn2+(aq), there is a solid formed. Which means that Zn2+ is getting reduced (to form the solid). This must also mean that Zn2+ has a higher reduction potential than Al(s). Does this conversely mean that Al(s) has a higher oxidation potential than Zn2+? And thus if you put the Al(s) into the same beaker with the HCl, it *must* reduce the H+ ions because we know that the oxidation potential is definitely higher than the Zn(s)?
Follow up questions:
If we look at the opposite reaction: Zn(s) + Al3+ (aq), nothing is formed. This means that Al3+ needs to be reduced, but it's not. Which means that Zn(s) has a higher reduction potential than Al3+ -- does this say anything about Al(s)???
I'm also a little confused why a metal with a higher oxidation potential will for sure make the HCl reaction spontaneous. There's some link I'm missing...
Also, does a higher oxidation potential mean a more negative E?
What I understand:
Zn(s) + HCl --> H2(g), which means that 1) H+ gets reduced and 2) the reaction is spontaneous. The question asks if a strip of Al(s) is placed in a beaker, will H2(g) evolve?
Then, we look at the table. We see that for Al(s) + Zn2+(aq), there is a solid formed. Which means that Zn2+ is getting reduced (to form the solid). This must also mean that Zn2+ has a higher reduction potential than Al(s). Does this conversely mean that Al(s) has a higher oxidation potential than Zn2+? And thus if you put the Al(s) into the same beaker with the HCl, it *must* reduce the H+ ions because we know that the oxidation potential is definitely higher than the Zn(s)?
Follow up questions:
If we look at the opposite reaction: Zn(s) + Al3+ (aq), nothing is formed. This means that Al3+ needs to be reduced, but it's not. Which means that Zn(s) has a higher reduction potential than Al3+ -- does this say anything about Al(s)???
I'm also a little confused why a metal with a higher oxidation potential will for sure make the HCl reaction spontaneous. There's some link I'm missing...
Also, does a higher oxidation potential mean a more negative E?