Which species will reduce I2 but not Sn4+?
Identify the species that undergoes oxidation inthe following reaction. H2O2 + Sn2+ à H2O + Sn4+ a) H2O2 b) Sn2+ c) H2O d) Sn4+
Which species will reduce Mn3+ to Mn2+ (Ecell = 1.51 V) but will NOT reduce Cr3+ to Cr2+ (Ecell = -0.40 V)? (Can you explain with steps on how to find the correct answer, and why the other answers are not correct?)
Given the following information calculate the equilibrium concentrations of all species. H2 + I2 = 2HI Kc=54.3 Initial [H2]=[I2]=.500 M, [HI]=0
Rank these species by their ability to act as an oxidizing agent. Cl2, I2, Mg2+, Fe2+
MnO4- + I− → Mn2+ + I2 in this equation, which is the oxidizing agent reducing agent species that has been reduced species that has been oxidized
Which of the following species can reduce Pb2+? See attached table!SRP.docx O a cu O b. Ag OC. Be2 O d. mg
Balance each of the following redox reactions occurring in acidic solution. 1. I−(aq)+NO−2(aq)→I2(s)+NO(g) 2. IO3−(aq)+H2SO3(aq)→I2(aq)+SO42−(aq) 3. NO−3(aq)+Sn2+(aq)→Sn4+(aq)+NO(g)
Half-reaction E° (V) I2(s) + 2e- 2I-(aq) 0.535V Pb2+(aq) + 2e- Pb(s) -0.126V Cr3+(aq) + 3e- Cr(s) -0.740V The strongest oxidizing agent is: ______enter formula The weakest oxidizing agent is: The weakest reducing agent is: The strongest reducing agent is: Will I2(s) reduce Cr3+(aq) to Cr(s)? Which species can be reduced by Pb(s)? If none, leave box blank.
which of the following spontaneous reactions is associated with the cell, Pt(s)l Sn2+,Sn4+ll Ag+ l Ag(s) a)Aq + e---> Ag+ c)Pt + 2e- --> Pt2- d)sn4+ + Ag+ --> Pt2+ Ag(s) + Sn2+ e) none of the above
Please help. I'm not sure how to go about figuring out which species oxidize or reduce or which are the agents. 2. Complete the table given that the following three reactions occur in the direction as written: a) 2Ag' (aq) + Fe(s) - Fe?' (aq) + 2Ag (s) b) 2Ag (aq) + Cu(s) — Cu (aq) + 2Ag (s) c) Cu (aq) + Fe (s) - Fet (aq) + Cu(s) Reaction Species oxidized Species reduced Oxidizing agent Reducing agent 3....