Write a balanced net-ionic equations to describe a. reduction of Fe3+ to fe2+ by SO2 b. reaction of H2MoO4 in a Jones reductor c. oxidation of HNO2 by a solution of MnO4- d. reaction of aniline (C6H4NH2) with a mixture of KBrO3 and KBr in acidic solution e. air oxidation of HAsO3(2-) to HAsO4(2-) f. reaction of KI with HNO2 in acidic solution

Write a balanced net-ionic equations to describe a. reduction of Fe3+ to fe2+ by SO2 b. reaction of H2MoO4 in a Jones reductor c. oxidation of HNO2 by a solution of MnO4- d. reaction of aniline (C6H4NH2) with a mixture of KBrO3 and KBr in acidic solution e. air oxidation of HAsO3(2-) to HAsO4(2-) f. reaction of KI with HNO2 in acidic solution

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter14: Applications Of Ultraviolet-visible Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 14.7QAP: A 3.03-g petroleum specimen was decomposed by wet ashing and subsequently diluted to 500 mL in a...

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Write balanced net-ionic equations to describe: (a) the reduction of Fe3+ to Fe2+ by SO2 (b) the reaction of H2MoO4 in a Jones reductor (c) the oxidation of HNO2 by a solution of MnO-4. (d) The reaction of aniline (C6H4NH2) with a mixture of KBrO3 and KBr in acidic solution (e) the air oxidation of HAsO2-3 to HasO2-4 (f) the reaction of KI with HNO2 in acidic solution Please answer letters d, e, and f
Write balanced net-ionic equations to describe: (a) the reduction of Fe3+ to Fe2+ by SO2 (b) the reaction of H2MoO4 in a Jones reductor (c) the oxidation of HNO2 by a solution of MnO-4. (d) The reaction of aniline (C6H4NH2) with a mixture of KBrO3 and KBr in acidic solution (e) the air oxidation of HAsO2-3 to HasO2-4 (f) the reaction of KI with HNO2 in acidic solution
Consider the reaction between dissolved Fe2+ and elemental sulfur (S0) to form hematite (Fe2O3) and sulfide a) Identify the oxidant and reductant in this reaction, determine half-reactions, and balance thereaction. b) Is this reaction thermodynamically favorable? c) Would you expect HS- to react readily with Fe2O3 (i.e. the reverse of the reaction)?
1. Account for the fact that [SiF6]-2 is a well-known species, while the corresponding [CF6]-2 does not exists. 2. Arrange the following oxides K2Cr2O7, Cr2O3 and CrO in order of increasing oxidizing power. Write the oxidation states of Cr in each compound. 3. Which is more easily hydrolysed CCl4 or SiCl4? Explain your answer.
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1. A Cr3+ solution is electrolyzed using a current of0.365 A. What mass of Cr(s) (51.9661) is plated outafter 10 hours?2. When an aqueous solution of CuSO4 is electrolyzedcopper metal is deposited. If a constant current waspassed for 5.00 h and 404 mg of Cu (63.546) metal wasdeposited, what was the current?
Compare the energetic favorability of MnO2 reduction by sulfide yielding S0 to the energetic favorability of MnO2 reduction by sulfide yielding SO42-. use numbers...no words to explain
Given A, B, and C… [A] U(VI) as uraninite; UO2 (where Fe2+= reductant; Fe(OH)3 ferrihydrite= product): 2Fe2+ + UO22+ +3H2O + H+ ---- > 2Fe(OH)3 + U4+ +2H2O [B] U(VI) as uraninite; UO2 (where Mn2+= reductant; MnO2 pyrolusite= product): 2H2O + UO22+ + Mn2+ ---- > UO2 + B - MnO2 + 4H+ [C] U(VI) as as uraninite; UO2 (where HS-= reductant; S0= product): UO22+ + Hs- ---- > UO2 + S + H+ QUESTION: Use thermodynamic calculations [use redox potential (Eh)] to predict which of the three reductants below is most favorable at pH 3 ? (1) Fe2+ (2) Mn2+ (3) HS-
if we use KMnO4 and H3Po4 and MnSO4 for tritation of fecl3 and calculation of. Fe2+ what suitable ratio for tritation
1. What are the practical implications of alloying in carbon and alloy steels? 2. Make use of drawings of segments of the Fe-Cr phase diagram to illustrate the reason for the existence offerritic, martensitic and austenitic stainless steels by also noting the influence of specific alloying elementswhere-applicable. .
A 0.703 g sample of a commercial detergent was red-calcined to destroy its components. organic. Treatment of the residue with hot HCl gave phosphorus in solution as H3PO4. the phosphate was precipitated as MgNH4PO4-6H2O by the addition of Mg + 2 or followed by aqueous NH3. The precipitate was filtered, washed, and converted to Mg2P2O7 by calcination at 1000 C. The residue weighed 0.432 g. Calculate the percentage of phosphorus in the sample.
1-Why σ2px lie at higher energy level than π2py and π2pz in N2? 2-Discuss the structure of [Ni (CN)6]-2 on base of VBT