2. Consider reaction-4 in the procedure: (a) How is the reaction between MnO4 and I in basic solution different from the one in acidic solution? What is the distinctive color formed in the cyclohexane layer for the reaction in acidic solution?

The Latimer Diagram of Cr ions is show below 0.55 1.34 2.10 - 0.424 - 0.90 Cr,0 Cr(v) → Cr(iv) → Cr(1) Cr(11) Cr 1.38 - 0.74 a.) What is the E° for the reduction of Cr2O,2 to Crt. Show your calculation b.)What is the E° for the reduction of CrO, to Cr** and Cr* to Cr**. Show your calculation. c.) From the given Latimer diagram construct a Frost diagram. Show your calculations and predict what Cr species will undergo disproportion and predict the product of the reaction.

Below are the reduction half reactions for chemolithoautotrophic nitrification, where ammonia is a source of electrons and energy and oxygen is the terminal electron acceptor. NO2- + 6e- -> NH4+ (E0 = +0.34 volts) O2 + 4e- ->  2H2O (E0 = +0.82 volts) If you balance and combine the reactions so that 293 moles of NH4+are oxidized to NO2-, how many moles of electrons will be transferred from Nitrogen to Oxygen?

as XC O What is the oxidation half-reaction (after equalizing electrons) for the redox reaction below? Hints: This equation covalent species; chlorine has an oxidation state of -1 in each of the compounds shown below. 2 TICI4 + H2 --> 2 TİCI3 + 2 HCI 1) A pure ("free") element has an oxidation state of 0. 2) The oxidation state for a monatomic ion (e.g. Ca2+, S2-) is equal to the ion charge. 3) Fluorine has an oxidation state of-1 in all of its compounds. 4) Hydrogen has an oxidation state of +1, except when it is combined with metals (-1). 5) Oxygen almost always has a -2 oxidation state. 6) Chlorine, bromine, and iodine have a -1 oxidation state, except when combined with fluorine or oxygen.* O2 Tit-> 2 Ti + 2 e OH2 + 2 e --> 2 H* O H - 2 H* + 2e 4 C- 3 CI + e 2 Ti + 2 e-- 2 Ti DELL increasing priority

In the following oxidation-reduction chemical reaction which chemical species is getting reduced? Hint: Oxygen oxidation number is -2 in Cr207 (ag)and -1 in H2O2(aq) and 0 in O2(g). Hydrogen oxidation number is +1. 2- %3D O2(3) Cr3+ (aq) H2O2(aq) + Cr2O,2 ag)

A group of students were tasked to perform the metal coupling of iron nail similar to Experiment 3: Corrosion of Metals. They were given two metals, metal Q and metai J, to couple to iron nail. They prepared an agar medium with KgFe(CN); and phenolphthalein. Their professor informed them that metal Q forms an orange color while metal J forms maroon color when oxidized. Their professors also gave them the reduction half-reactions for the corresponding metal ions including the reduction of Fe 12+ 2e -) Fe* + 2e- Fe E° =- 1.66 v E° = - 0.44 v Q2- + 2e-Q O2 + 2H20 + 4e- 40H* What color in the set-up indicates reduction process for Fe nail coupled with metal Q? E° =.0.25 v E° = + 0.40 v A pink B) orange blue maroon

Provide the balanced chemical equation for the undesirable reaction between HgCl2 and Sn2+ that will occur if you use too much Sn2+ during the reduction step (forms a gray precipitate).

46 Solution of hydrogen sulfite was added to a solution of potassium dichromate. H2SO3 + Cr2072- Cr3+ + SO42- pr the reaction above: Relate the observations to the species involved Write balanced half equations and the overall equation for the reaction Identify with reasons the oxidant and the reductant in terms of change in oxidation number or electron transfer.

Predict whether reaction would proceed spontaneously or not for the following system at 298 K and write net reaction for each? Write the net equation for each sample. (Please found Standard redox potential yourselves) Metallic Au in 1 M HNO3 Metalic Mn in water