Hello, I am currently doing a practice exam (not for a grade, just practice) and am somewhat confused on how to do the second question, it states: Consider a galvanic cell constructed from (Cu^2+/Cu) and (Fe^3+/Fe^2+) half-cells. The half-cells are connected with a KNO3 salt bridge. One of the electrodes is platinum (Pt) and one is made out of another metal. a) Identify the oxidizing agent and the reducing agent. We are given a formula sheet and the formula sheet includes the following half-reactions: Fe3+ + e- = Fe2+ v= 0.77 Cu2+ + 2e-= Cu v= 0.34 Fe3+ + 3e- = Fe v= -0.036 Fe2+ + 2e- = Fe v= -0.44 For part a the answer is: oxidizing agent= Fe3+ (it gets reduced) reducing agent= Cu (it gets oxidized) but I am confused as to how this is the answer. For part b the question is: Write a balanced chemical reaction for the process. The answer is: Cu + (2Fe^3+) --> Cu^2+ + 2Fe^2+ I just need an explanation for how this is the answer. For part C the question is: Calculate the E for this spontaneous process. 0.77v- 0.34v = 0.43 v I am somehwat confused how to get this value. Part d states: In the following sketch, label the electrodes and species in each solution. Indicate the movement of all the ions and electrons, including those of the salt bridge, in the galvanic cell. Show: i. Which reaction is happening at which electrode. ii. The direction of electron flow. iii. The flow of ions from the slat bridge. iv. What metal each electrode is made of. The sketch is on the answer key, but I just need an explanation as to how to do it. Part e states: Explain what happens to each of the following as the reaction proceeds: -Cu electrode -Pt electrode -[Cu^2+] -[Fe^2+] -[Fe^3+] -Ecell
Hello,
I am currently doing a practice exam (not for a grade, just practice) and am somewhat confused on how to do the second question, it states:
Consider a galvanic cell constructed from (Cu^2+/Cu) and (Fe^3+/Fe^2+) half-cells. The half-cells are connected with a KNO3 salt bridge. One of the electrodes is platinum (Pt) and one is made out of another metal.
a) Identify the oxidizing agent and the reducing agent.
We are given a formula sheet and the formula sheet includes the following half-reactions:
Fe3+ + e- = Fe2+ v= 0.77
Cu2+ + 2e-= Cu v= 0.34
Fe3+ + 3e- = Fe v= -0.036
Fe2+ + 2e- = Fe v= -0.44
For part a the answer is:
oxidizing agent= Fe3+ (it gets reduced)
reducing agent= Cu (it gets oxidized)
but I am confused as to how this is the answer.
For part b the question is:
Write a balanced
The answer is:
Cu + (2Fe^3+) --> Cu^2+ + 2Fe^2+
I just need an explanation for how this is the answer.
For part C the question is:
Calculate the E for this spontaneous process.
0.77v- 0.34v = 0.43 v
I am somehwat confused how to get this value.
Part d states:
In the following sketch, label the electrodes and species in each solution. Indicate the movement of all the ions and electrons, including those of the salt bridge, in the galvanic cell.
Show:
i. Which reaction is happening at which electrode.
ii. The direction of electron flow.
iii. The flow of ions from the slat bridge.
iv. What metal each electrode is made of.
The sketch is on the answer key, but I just need an explanation as to how to do it.
Part e states:
Explain what happens to each of the following as the reaction proceeds:
-Cu electrode
-Pt electrode
-[Cu^2+]
-[Fe^2+]
-[Fe^3+]
-Ecell
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