26.4 Complete and balance the following reaction, then give the product side of the balanced equation. Zn (s) + FeCl3 (aq) → Select one: a. no Reaction b. None of these C. ZnCl2 (aq) + Fe (s) d. ZnCl3 (aq) + Fe (s) e. 3 ZnCl2 (aq) + 2 Fe (s) f. ZnFe (aq) + Cl2 (g) g. ZnFeCl2 (aq) + Fe (s) h. ZnCl2 (s) + Fe (s)

26.4 Complete and balance the following reaction, then give the product side of the balanced equation. Zn (s) + FeCl3 (aq) → Select one: a. no Reaction b. None of these C. ZnCl2 (aq) + Fe (s) d. ZnCl3 (aq) + Fe (s) e. 3 ZnCl2 (aq) + 2 Fe (s) f. ZnFe (aq) + Cl2 (g) g. ZnFeCl2 (aq) + Fe (s) h. ZnCl2 (s) + Fe (s)

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter19: Transition Metals And Coordination Chemistry

Section: Chapter Questions

Problem 15E: The standard reduction potential for the reaction [Co( H 2 O)6]3+(aq)+e[CO( H 2 O)6]2+(aq) is about...

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The standard reduction potential for the reaction [Co( H 2 O)6]3+(aq)+e[CO( H 2 O)6]2+(aq) is about 1.8 V. The reduction potential for the reaction [Co( NH 3 )6]3+(aq)+e[Co( NH 3 )6]2+(aq) is +0.1 V. Calculate the cell potentials to show whether the complex ions,. [Co( H 2 O)6]2+ and or [Co( NH 3 )6]2+, can be oxidized to the corresponding Cobalt (III) complex by oxygen.
(a) What is the percentage of MnO2 in a pyrolusite ore if a sample weighing 0.4000g is treated with 0.6000g of pure H2C2O4•2H2O and dilute H2SO4 and after reduction has taken place (MnO2 + H2C2O4 + 2H+→ Mn2++ 2CO2 + 2H2O), the excess oxalic acid requires 26.26ml of 0.1000N KMnO4 for titration? (b) If pure As2O3 were used instead of oxalic acid, how many grams would be required in order for the other numerical data to remain the same?
(a) What is the percentage of MnO2 in a pyrolusite ore if a sample weighing 0.4000 g is treated with a 0.6000 g of pure H2C2O4.2H20 and dilute H2SO4 and after reduction has taken place (MnO2 + H2C2O4 + 2H+ Mn2+ + 2CO2 + 2H2O), the excess oxalic acid requires 26.26 mL of 0.1000 N KMNO4 for titration? (b) If pure As2O3 were used instead of oxalic acid, how many grams would be required in order for the other numerical data to remain the same?
A sample of pyrolusite weighing 0.6000 g is dissolved in a solution containing 5.00mL of 6.00 N H2SO4 and 0.900 g of H2C2O4.2H2O. The excess oxalate then requires24.00 mL of KMnO4 solution for titration. If each mL of the KMnO4 will oxidize the Fe(II)in 0.03058 g FeSO4.7H2O, what is the oxidizing power of the sample in terms of MnO2?84.33%
A Chemist collected a 0.4891-g sample of an ore for Fe determination by a redox titration with K2Cr2O7.The ore was carefully crushed prior to weighing and dissolved in HCl and using a Jones reductor the ironin the sample was brought into the +2 oxidation state. After titration with diphenylamine sulfonic acid,itrequired 36.92 mL of 0.02153 M K2Cr2O7 to reach the end point. Show your solution why 77.86% is the iron content of the ore as %w/w Fe2O3.
A Chemist collected a 0.4891-g sample of an ore for Fe determination by a redox titration with K2Cr2O7.The ore was carefully crushed prior to weighing and dissolved in HCl and using a Jones reductor the ironin the sample was brought into the +2 oxidation state. After titration with diphenylamine sulfonic acid,itrequired 36.92 mL of 0.02153 M K2Cr2O7 to reach the end point. Calculate the iron content of the ore as%w/w Fe2O3
A sample of pyrolusite weighing 0.6000 g is dissolved in a solution containing 5.00 mL of 6.00 N H2SO4 and 0.900 g of H2C2O4 .2H2O. The excess oxalate then requires 24.00 mL of KMnO4 solution for titration. If each mL of the KMnO4 will oxidize the Fe(II) in 0.03058 g FeSO4 .7H2O, what is the oxidizing power of the sample in terms of MnO2?
A sample of steel weighing 2.00 g is analyzed for Cr (AW 52.0). The Cr is oxidized into chromate with alkaline permanganate and the excess permanganate is destroyed. A certain volume of 0.120 M FeSO4 is added to the acid solution and the excess is titrated with 0.0220 M KMnO4, requiring 31.0 mL. If the sample contained 0.50 % Cr, what volume (in mL) of FeSO4 was added?
What is the % of Cr in a sample of chrome-iron ore if 0.200 g of the ore after oxidation with Na2O2 and treatment of the acidified solution with 5.0 mmol of ferrous sulfate requires 0.166 mmol of dichromate for the x’ss Fe(II)?
Given the metal activity trend below. Al > Cr > Ni > H2 > Pt Which of the following will reduce Cr2+ to Cr? a. Cr metal b. Al metal c. Ni metal d. H2 gas
A pure oxide of iron weighing 1.000 g is fused with K2S2O7 and the fused material dissolved in acid. The Fe3+ is reduced with SnCl2, HgCl2 is added, and the Fe2+ titrated with 0.1667 M K2Cr2O7 solution, requiring 12.96 mL. What was the formula of the original oxide?
A pure oxide of iron weighing 1.000 g is fused with K2S2O7 and the fused material dissolved in acid. The Fe3+ is reduced with SnCl2, HgCl2 is adthe Fe2+ titrated with 0.1667 M K2Cr2O7 solution, requiring 12.96 mL. What was the formula of the original oxide? FeO Fe3O4 Fe2O3Fe2O