Consider the following balanced reaction: 2MnO4^- (aq) + 2H+ (aq) + 3SO3^2- (aq) —> H2O (l) + 2MnO2 (s) + 3SO4^2- (aq) A: Mn B: O C: S D: H E: MnO4^- F: H+ G: SO3^2- For each, decide if they are either of the listed below: 1. Neither oxidized nor reduced 2. Is oxidized 3. Is reduced 4 . Is the oxidizing agent 5. Is the reducing agent 6. Is neither the oxidizing agent nor the reducing agent

Consider the following balanced reaction: 2MnO4^- (aq) + 2H+ (aq) + 3SO3^2- (aq) —> H2O (l) + 2MnO2 (s) + 3SO4^2- (aq) A: Mn B: O C: S D: H E: MnO4^- F: H+ G: SO3^2- For each, decide if they are either of the listed below: 1. Neither oxidized nor reduced 2. Is oxidized 3. Is reduced 4 . Is the oxidizing agent 5. Is the reducing agent 6. Is neither the oxidizing agent nor the reducing agent

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 29Q: When jump-starting a car with a dead battery, the ground jumper should be attached to a remote part...

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In an analysis of metal carbonate M2CO3∙3H2O, 1.500g of the unknown carbonate was dissolved in enough water to make a 100.0mL solution. 20.00mL of such solution was treated with 10.00mL of 1.000M HCl solution, and the excess acid was titrated with 54.92mL of 0.1138M NaOH solution. The equations are given below: CO32-(aq) + 2 H+(aq) → H2O(l) + CO2(g) H+(aq) + OH-(aq) → H2O(l) a) the moles of NaOH used in the titration is (enter the answer in 4 sig. figs.) Answer mol b) the mole of HCl reacted with the carbonate is (enter the answer in 4 sig. figs.) Answer mol c) the molar mass of M2CO3∙3H2O is (enter the answer in 4 sig. figs.) Answer g/mol d) the identity of metal M is (enter the element symbol) Answer
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if 361.3 mg of Li2(SO4) (FW=109.95) is added to 450 mL of 0.828 M NH4F, what is the Qip for lithium fluoride. (Ksp of lithium fluoride= 3.8 x10^-3)
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3I- + OCl- + 2H+ ----> I3- + Cl- + H2: A 25.00 ml sample of liquid bleach was diluted to 1000 ml in a graduated flask. A 25 ml portion of the diluted sample was pipetted into an Erlenmeyer flask and treated with excess KI to oxidize OCl- to Cl- and I3- was produced at the end of the reaction. The released I3 was titrated with 0.09892 M Na2S2O3 and 8.96 ml was spent to reach the turning point besides the starch indicator. What is the percent by weight/volume of NaOCl in the bleach sample? (NaOCl:74.44 g/mol)
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So I am given the reaction Fe3++SCN-→←Fe(SCN)2+. [Fe3+]i = 0.0018 M , and [Fe(SCN)2+]eq = 3.206 x 10-5 M . How do I solve for [Fe3+]eq ? I also have that [SCN-]i=0.0020 M, but I do not know if it is relevant.