For there reaction system involving the species in the table below, what conclusion is
justified for standard state conditions?
Standard Reduction Potentials E0
2Fe3+ + Sn2+ ¡ú 2Fe2+ + Sn4+ +0.62 V
Sn2+ + I2 ¡ú Sn4+ + 2I¨C +0.38 V
(A) I¨C would react with Fe3+
(B) Fe2+ would react with I2
(C) Fe3+ is a weaker oxidizing agent than I2
(D) Fe2+ is a stronger reducing agent than I¨C
My screen is gibberish again on both .
I'm wondering if you are using a Mac.
2Fe3+ + Sn2+ ¡ú 2Fe2+ + Sn4+ +0.62 V
Sn2+ + I2 ¡ú Sn4+ + 2I¨C +0.38 V
man this sucks well hold on
2Fe3+ + Sn2+ --> 2Fe2+ + Sn4+ +0.62 V
Sn2+ + I2 --> Sn4+ + 2I– +0.38 V
i hope this is better
Yes. That's better but I don't have time to look at it now. I'll get back later.
But you also need to redo the answers because they contain some of the same strange symbols. especially the A answer.
To determine the conclusion justified for standard state conditions, we need to analyze the standard reduction potentials (E0) of the given species.
In the table, we have two redox reactions with their respective standard reduction potentials:
1. 2Fe3+ + Sn2+ → 2Fe2+ + Sn4+ E0 = +0.62 V
2. Sn2+ + I2 → Sn4+ + 2I- E0 = +0.38 V
The standard reduction potential (E0) represents the tendency for a species to be reduced (gain electrons). A more positive E0 value indicates a stronger tendency to be reduced.
Now, let's analyze the reactions:
1. In the first reaction, Fe3+ is being reduced to Fe2+ with Sn2+ acting as the oxidizing agent. The positive E0 value of +0.62 V suggests that Fe3+ is a stronger oxidizing agent than Sn2+. Therefore, Fe3+ has a greater tendency to accept electrons and be reduced compared to Sn2+.
2. In the second reaction, Sn2+ is being oxidized to Sn4+ with I2 acting as the reducing agent. The positive E0 value of +0.38 V indicates that I2 is a stronger oxidizing agent than Sn2+. Therefore, I2 has a greater tendency to gain electrons and be reduced compared to Sn2+.
Based on the analysis, we can conclude:
(A) I- would react with Fe3+: This conclusion is not justified as the E0 values do not provide information about the reactivity of I- with Fe3+. We cannot determine the reactivity between these two species with the given data.
(B) Fe2+ would react with I2: This conclusion is not justified as the E0 values suggest that I2 has a greater tendency to be reduced compared to Fe2+.
(C) Fe3+ is a weaker oxidizing agent than I2: This conclusion is justified as the positive E0 value for I2 (+0.38 V) indicates that it is a stronger oxidizing agent compared to Fe3+ (+0.62 V).
(D) Fe2+ is a stronger reducing agent than I-: This conclusion is not justified as the E0 values do not provide information about the reactivity between Fe2+ and I-.
Therefore, the correct conclusion justified for standard state conditions is:
(C) Fe3+ is a weaker oxidizing agent than I2.