a) Will Al(s) react with a 1 M tin(IV) solution?
b) Will 1 M Fe2+ react with Sn(s)?
Sn4+ + 2 e- → Sn2+ (s) +0.15 V
Sn2+ + 2 e- → Sn (s) -0.14 V
Fe2+ + 2 e- → Fe (s) -0.44 V
Al3+ + 3 e- → Al (s) -1.66 V
please explain step by step how to determine this. this is electrochemistry
a) Will Al(s) react with a 1 M tin(IV) solution? b) Will 1 M Fe2+ react...
consider the following standard reduction potentials. Reduction Half-Reaction Eo (volts) Al3+(aq) + 3e− → Al(s) − 1.66 Fe2+(aq) + 2e− → Fe(s) − 0.44 Sn2+(aq) + 2e− → Sn(s) − 0.14 The Al/Al3+ half-reaction can be paired with the other two to produce voltaic cells because ________ A) Al is a more powerful oxidizing agent B) Fe and Sn are readily oxidized Al is a more powerful reducing agent C) Al3+ is a more powerful oxidizing agent D) Al3+...
Consider the following standard reduction potentials in acid solution:E^o(V)Al3+ + 3e– ? Al(s) –1.66AgBr(s) + e– ? Ag(s) + Br– +0.07Sn4+ + 2e– ? Sn2+ +0.14Fe3+ + e– ? Fe2+ +0.77The strongest reducing agent among those shown above is
pls explain in great detail why Consider the following standard reduction potentials Reduction Half-Reaction A1+ (aq) + 3e A1(s) Fe2+ (aq) + 2e-Fe(s) Sn2+ (aq) + 2e - Sn(s) E (volts) -1.66 0.44 0.14 The AIAP half-reaction can be paired with the other two to produce voltaic cells because Als* is a more powerful reducing agent OOO Al is a more powerful oxidizing agent o Fe and Sn are readily oxidized Al is a more powerful reducing agent AB+ is...
Half-reaction Cr3+ (aq) + 3e- → Cr(s) Fe2+ (aq) + 2e- → Fe (s) Fe3+ (aq) + e- + Fe2+ (s) Sn4+ (aq) + 2e- + Sn2+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154 3Sn** (aq) +2Cr(s) → 2Cr** (aq) +3Sn²+ (aq) 3. What is the cell potential, Ecell, for the reaction above if [Sn] = 1.00 M, [Cr3+1 = 0.0200 M and [Sn2+] = 0.0100 M?
pls explain very detailed on how to do this question Question 6 Consider the following standard reduction potentials. Reduction Half-Reaction A13+ (aq) + 3e-Al(s) Fe2+(aq) + 2e-Fe(5) Sn2+ (aq) + 2e - Sn(s) E' (volts) + 1.66 -0.44 - 0.14 The Al Al half-reaction can be paired with the other two to produce voltaic cells because
Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. a Fe electrode in 1.0 M FeCl2 solution a Sn electrode in 1.0 M Sn(NO3)2 solution Fe2+ + 2e- → Fe Eo = -0.44 V Sn2+ + 2e- → Sn Eo = -0.14 V When the cell is running spontaneously, which choice includes only true statements and no false ones? Select one: a. The iron electrode gains mass and the iron electrode is the...
ans A C B how ? 14. Consider the titration of 25.00 mL of 0.0500 M Sn2+ with 0.100 M Fe3+ in 1 M HCl to give Fe2+ and Sn4+, using Pt and saturated calomel electrodes SCE l Sn4+, Sn2+, Fe3+, Fe3 | Pt(s) The titration reaction: 2Fe3 + Sn2+Snt+ 2Fe2+ The two half-reactions for the indicator electrode: Fe3+e Sn 2e Sn2+ Indicate the two Nernst equations for the cell voltage. E 0.732 V E 0.139 V Fe2+ IFe2 log...
Have I done these correctly? Which of the options below correctly describes what happens when a small amount of water is added to a buffer solution consisting of the weak acid HA its conjugate base A? a. The concentration of HA remains the same and the concentration of Hincreases. O b. The concentration of HA remains the same and the concentration of H* decreases. O c. The concentration of HA increases and the concentration of Ht remains the same. d....
Identify the reducing agent. 2 Al3+(aq) + 2 Fe(s) = 2 Al(s) + 3 Fe2+(aq) A) Fe B) Al C) Fe2+ D) Al3+ E) This is not an oxidation-reduction reaction.
Question 3 Calculate the E if the concentration of Zn2+ = 1.5 M and Fe2+ = 0.5 M. Zn (S) + Fe2+ (aq) — Zn2+ (aq) + Fe (s) -0.44 0.83 Fe2+ (aq) + 2e — Fe(s) Zn (aq) + 2e2 Zn(s) 2 H,0() + 2e H2(g) + 2OH(aq) AP(aq) + 3e Al(s) Na (aq) + e L" (aq) + e -1.66 -2.71 3.05 Question 4