5. Balance the following oxidation-reduction equations. All reactions occur in basic solutions.(a) S203² + OCI → SO² + Cr(b) NiO₂+ Fe → Ni(OH)2+ Fe(OH)3(c) SbH3 + H₂O → Sb(OH)4 + H₂(d) P4 PH3 + HPO3²-

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Answered: 5. Balance the following…

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Complete and balance the following redox reaction in basic solution CIO3 (aq) + C204² (aq) → CIO2(g) + CO2(g) 14- 3- |2- O2+ 3+ 4+ 1 6. 7 8 9 0. O3 Os O, Do 12 14 7 9. (s) (1) (g) (aq) OH H2O ei H3O 4+ 2. +
8. How many grams of N.H2PO4 are needed to completely neutralize 33.65 mL of a 0.129 M NaOH solution? (a) Balance this equation first: 1 NaH, PO4(s) + 2v NaOH (aq) - 1 v Na3PO4(aq) + 2 H2O(I) → (b) Answer:
BALANCE THE FOLLOWING OXIDATION-REDUCTION REACTIONS OCCURRING IN ACIDIC SOLUTION USING THE HALF-REACTION METHOD. 1. CH;OH(aq) + Cr2O,²- (aq) CH20(aq) + Cr³+(aq) 2. As2O3(s) + NO;(aq) H3ASO4(aq) + NO(g)
The following skeletal oxidation-reduction reaction occurs under acidic conditions. Write the balanced OXIDATION half reaction. Co2+ + NO Co + NO3-
Given the following half-reactions, 2 103 (aq) + 12H*(aq) + 10 e → 12(s) + 6H2O Fe2* (aq) → Fe3* (aq) + e" write the balanced overall reaction. 2103 - (aq) + 12 H* (aq) + Fe 2* (aq) → Fel2 (s) + 6 H2O o 2 103 (aq) + 10 Fe²* (aq) → l2 (s) + 10 Fe³+ (aq) 2 103 - (aq) + 12 H* (aq) + Fe 2* (aq) → 12 (s) + Fe3+ (aq) + 6 H20 2 103 - (aq) + 12 H* (aq) + 10 Fe 2* (aq) → 12 (s) + 10 Fe3+ (aq) + 6 H20
Balance the following redox reaction under acidic conditions. H2O2(aq) + Cl2O7(aq) = ClO2-(aq) + O2(g)
Consider the following redox reaction: Ag⁺(aq) + Fe²⁺(aq) ⇌ Ag(s) + Fe³⁺(aq). What quantity in moles of electrons are exchanged?
2. Indicate whether the following balanced equations involve oxidation-reduction. If they do, identify the elements that undergo changes in oxidation number (a) PB13 ) + 3 H2O () → H3PO3 (ag) + 3 HBr@g) (b) Nal (aa) + 3 HOCI99) –→ NaIO3(ag) + 3 HCl (99) (c) 3 SO2 (2 + 2 HNO3(aq) + 2 H2O () → 3 H2SO4aq) + 2 NO (2) (d) 2 AgNO3(q) + CoCl2(a@) + → 2 AgCl (6) + Co(NO3)2 (aa) + 000 oG titeniuma totue hlouid fomm c lid tite
Balance the following oxidation-reduction reactions. acidic solution a. PbO₂+ Hg-Hg2+ Pb²+ b. NO3(aq) + H2(g) → NO) + H₂O(1) basic solution
Complete and balance the following redox reaction in basic solution 2- 3c₂²- 1 + 2 (s) H* CIO₂(g) →CIO₂ (aq) + CIO3(aq) 3 4 H₂O Reset ( (1) LO 5 OH- H 6 (g) H3O+ 7 8 CI • x H₂O 9 (aq) S
Write a balanced chemical equation for the following reaction in a basic solution.ClO–(aq) + Cr(OH)3(s) → Cl–(aq) + CrO42–(aq)
Balance the following redox reactions occurring in basic aqueous solution. Identify the species being oxidized, species being reduced, the oxidizing agent, and the reducing agent. ClO- (aq)+Cr(OH)4- > CrO4- + Cl-

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5. Balance the following oxidation-reduction equations. All reactions occur in basic solutions. (a) S203² + OCT → SO4² + Cr (b) NiO₂+ Fe → Ni(OH)2+ Fe(OH)3 SbH3 + H₂O → Sb(OH)4 + H₂ (d) P4 PH3 + HPO 3²-