***galvanic cell issue*** (1 Viewer)

[Lucas_]

I'm currently having a serious issue with (re)learning galvanic cells.

From the activity series, we know that a more active metal will displace a less active metal in solution, turning from an element into an ion + free electrons. We know that the less active element (currently in solution as ions) will accept those "donated" electrons to become solid residue.

In a galvanic cell I don't understand why, when placed in zinc sulfate solution, the zinc anode (negative because it's losing electrons) 'feels inclined' to turn into Zn ions and spare electrons. I could understand if it was placed in a copper ion solution or something....?

Worst part is that I completely understood this a few months; FML!

Thanks in advance

 

[someth1ng]

Okay, so, this is a galvanic cell. They are two separate half cells connected by a salt bridge and a lead with a device such as a light bulb or a voltmeter. The two half cell are hence, linked together. Now, the copper ions will have a tendency to "accept" electrons and the zinc ions will have a tendency to "donate" electrons. For this to occur, the copper cathode "pulls" electrons through the lead from the zinc anode.

 

[someth1ng]

View attachment 25952

Okay, so, this is a galvanic cell. They are two separate half cells connected by a salt bridge and a lead with a device such as a light bulb or a voltmeter. The two half cell are hence, linked together. Now, the copper ions will have higher tendency to "accept" electrons and the zinc ions will have a higher tendency to "donate" electrons. This results in the copper cathode to accept electrons from the zinc anode.