Class notes
Electrode potential
- Course
- Institution
Written with Virtual high school (VHS)
[Show more]
Seller
Follow
studystar9touni
Content preview
+ +1a) Ag(s)/𝐴𝑔 (aq) ‖ 𝐻 (aq)/H2(g):
Step 1 - Write 2 redox half reactions:
The oxidation half reaction is Ag(s) → Ag+ (aq) + e-.
The reduction half reaction is H+ (aq) + 2e- → H2(g).
Step 2 - Find E° reduction:
2H+ (aq) + 2e- → H2(g) E° = +0 V
Step 3 - Find E° oxidation using sign reversal:
This is the reverse of your oxidation reaction:Ag+ (aq) + e- → Ag(s)
Use the potential from the chart to determine E° oxidation: Ag+ (aq) + e- → Ag(s) E° = +0.80 V
To convert from reduction to an oxidation potential, reverse the sign:
E° oxidation = -E° reduction
= - (+0.80 V)
= - 0.80 V
Step 4 - Add the potentials to determine E° cell:
E° cell = E° reduction + E° oxidation
= (+ 0 V) + (- 0.80 V)
= +0 V - 0.80 V
= - 0.80 V
Therefore, the E° cell is - 0.80 V. Since the E° cell is a negative value, the reaction is
nonspontaneous.
Balanced net ionic equation:
+ +
2𝐴𝑔(𝑠) + 2𝐻 (𝑎𝑞) → 2𝐴𝑔 (𝑎𝑞) + 𝐻2(𝑔)
+ 2+
b) H2(g)/𝐻 (aq) ‖ 𝑍𝑛 (aq)/Zn(s):
Step 1 - Write 2 redox half reactions:
The oxidation half reaction is H2(g) → H+ (aq) + 2e-.
2+ −
The reduction half reaction is 𝑍𝑛 (𝑎𝑞) + 2𝑒 → 𝑍𝑛(𝑠).
Step 2 - Find E° reduction:
Zn2+ (aq) + 2e- → Zn(s) E° = -0.76 V
Step 3 - Find E° oxidation using sign reversal:
This is the reverse of your oxidation reaction: 2H+ (aq) + 2e- → H2(g)
Use the potential from the chart to determine E° oxidation: 2H+ (aq) + 2e- → H2(g) E° = + 0 V
To convert from reduction to an oxidation potential, reverse the sign:
E° oxidation = -E° reduction
= - (+ 0 V)
=-0V
Step 4 - Add the potentials to determine E° cell:
E° cell = E° reduction + E° oxidation
= (- 0.76 V) + (- 0 V)
= - 0.76 V -0V
= - 0.76 V
Therefore, the E° cell is - 0.76 V. Since the E° cell is a negative value, the reaction is
nonspontaneous.
Balanced net ionic equation:
2+ +
𝐻2(𝑔) + 𝑍𝑛 (𝑎𝑞) → 2𝐻 (𝑎𝑞) + 𝑍𝑛(𝑠)
The benefits of buying summaries with Stuvia:
Guaranteed quality through customer reviews
Stuvia customers have reviewed more than 700,000 summaries. This how you know that you are buying the best documents.
Quick and easy check-out
You can quickly pay through credit card or Stuvia-credit for the summaries. There is no membership needed.
Focus on what matters
Your fellow students write the study notes themselves, which is why the documents are always reliable and up-to-date. This ensures you quickly get to the core!
Frequently asked questions
What do I get when I buy this document?
You get a PDF, available immediately after your purchase. The purchased document is accessible anytime, anywhere and indefinitely through your profile.
Satisfaction guarantee: how does it work?
Our satisfaction guarantee ensures that you always find a study document that suits you well. You fill out a form, and our customer service team takes care of the rest.
Who am I buying these notes from?
Stuvia is a marketplace, so you are not buying this document from us, but from seller studystar9touni. Stuvia facilitates payment to the seller.
Will I be stuck with a subscription?
No, you only buy these notes for $6.25. You're not tied to anything after your purchase.
Can Stuvia be trusted?
4.6 stars on Google & Trustpilot (+1000 reviews)
67474 documents were sold in the last 30 days
Founded in 2010, the go-to place to buy study notes for 14 years now