Sketch the galvanic cell and determine the line notation for t...

Question

Sketch the galvanic cell and determine the line notation for the following redox reaction:

Ni²⁺ (aq) + Mg (s) ⇌ Ni (s) + Mg ²⁺ (aq)

Accepted Answer

So here we again, we have to sketch the galvanic cell and determine the line notation for the following redox reaction. Here, we have nickel 2+ion with an oxidation number of +2. It then goes to its natural or neutral form which gives us the oxidation number of 0. So it goes from being plus 2 to 0. So its oxidation number was reduced. Therefore, it represents the cathode. Then we have magnesium solid in its natural state so its oxidation number is 0. It goes to being a +2 charge. So now its oxidation number has increased. Therefore, it represents the anode where oxidation has occurred. If we draw our galvanic cell here, we have here our salt bridge. We have our electrode. Here, the solid electrode from my anode will represent the magnesium solid. We have our wire here which connects to our other solid electrode which, in this case, is the nickel electrode. We have our voltmeter here which reads the amount of voltage that's produced in terms of this galvanic or voltaic cell. The electrons are leaving my anode going towards the cathode. Through this process, we have the generation of magnesium ions. We have our negative ions traveling this way. We have some positive ions this way. Here we have the generation of nickel 2+ ions in this solution as well. Now if we're gonna talk about the line or cell notation, we'd first talk about our anode. So the lower oxidation state would be magnesium solid. Activity here approaches, unity which is 1. We have our phase boundary. Now we have our magnesium 2 ion. Here we have our actual break. Then we have our nickel 2+ ion. Our phase boundary. And that represents our line or cell notation in terms of of this galvanic cell. This one is a bit more simple. We didn't have to worry about the introduction of any outside gas being formed. But realize when we have gases involved, we typically would use some type of inert solid to react and act as our electrode within the redox reaction. In this one, because both we have both the magnesium solid and the nickel solid, there is no need to introduce any type of inert solid like platinum. So this would be a simple basic question to approach when it comes to line notation and the drawing of any galvanic or voltaic cell.

Struggling with Analytical Chemistry?

Sketch the galvanic cell and determine the line notation for the following redox reaction:
Ni²⁺ (aq) + Mg (s) ⇌ Ni (s) + Mg ²⁺ (aq)

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Struggling with Analytical Chemistry?

Sketch the galvanic cell and determine the line notation for the following redox reaction:Ni2+ (aq) + Mg (s) ⇌ Ni (s) + Mg 2+ (aq)

Watch next

Electrochemical Cells practice set

Sketch the galvanic cell and determine the line notation for the following redox reaction:
Ni²⁺ (aq) + Mg (s) ⇌ Ni (s) + Mg ²⁺ (aq)