For the following skeletal reaction, use the half-reaction method to write a balanced net reaction equation. The reaction occurs in acidic conditions. 1₂(aq) +S402(aq) - H₂SO3(aq) + I-(aq) In an acidic medium, the balanced oxidation half-reaction for the above reaction is: Select one: O S402(aq) + 9H+ (aq) → H₂SO3(aq) + 3H₂O(l) + 7e- O 1₂(aq) + 2e - 21-(aq) O S40²(aq) + 60H(aq) + 2H+ (aq) + 4H₂SO3(aq) + 7e- O S40²(aq) + 6H₂O(l) - 4H₂SO3(aq) + 4H+ (aq) + 6e- Select the correct coefficients for the hydrogen ions and the water molecules, as they appear in the balanced net reaction. Also indicate where both species appear in the net reaction equation. Entity Coefficient Side of reaction equation H+ (aq) H₂0 (1) I₂(aq) S402(aq) When the skeletal equation above is balanced using lowest whole numbers, the coefficients for each species is as follows: H₂SO3(aq) ◆ I-(aq) ◆ ◆

For the following skeletal reaction, use the half-reaction method to write a balanced net reaction equation. The reaction occurs in acidic conditions. 1₂(aq) +S402(aq) - H₂SO3(aq) + I-(aq) In an acidic medium, the balanced oxidation half-reaction for the above reaction is: Select one: O S402(aq) + 9H+ (aq) → H₂SO3(aq) + 3H₂O(l) + 7e- O 1₂(aq) + 2e - 21-(aq) O S40²(aq) + 60H(aq) + 2H+ (aq) + 4H₂SO3(aq) + 7e- O S40²(aq) + 6H₂O(l) - 4H₂SO3(aq) + 4H+ (aq) + 6e- Select the correct coefficients for the hydrogen ions and the water molecules, as they appear in the balanced net reaction. Also indicate where both species appear in the net reaction equation. Entity Coefficient Side of reaction equation H+ (aq) H₂0 (1) I₂(aq) S402(aq) When the skeletal equation above is balanced using lowest whole numbers, the coefficients for each species is as follows: H₂SO3(aq) ◆ I-(aq) ◆ ◆

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...

See similar textbooks

Similar questions

The iron content of foods can be determined by dissolving them in acid (forming Fe3+), reducing the iron(III) to iron(II), and titrating with cerium(IV): Fe2+(aq) + Ce4+(aq) → Fe3+(aq) + Ce3+(aq). Identify the two half-reactions in the above reaction. A) oxidation half-reaction. reduction half-reaction Fe2+(aq) + e-→ Fe3+(aq) Ce4+(aq) → Ce3+(aq) + e-
Balance the following redox reaction in basic solution. 2+ Cr(OH)3(s)+Fe³+ (aq) Cro² (aq) + Fe²+ (aq) 3+ 2+ Cr(OH), (s) + Fe³+ (aq) → Cro² (aq) + Fe²+ (aq) ロ→ロ X 40 5
For the following reaction, write the half-reactions and state which is the reduction and which is the oxidation half-reaction also identify the oxidizing agent and the reducing agent.
Write two half-reactions to describe each of these metal displacement reactions. Include phase symbols. Mg(s) + CoBr₂(aq) → MgBr₂(aq) + Co(s) - oxidation half-reaction: reduction half-reaction: Cu(s) + 2 AuCl(aq) → CuCl₂(aq) + 2 Au(s) 1 oxidation half-reaction: reduction half-reaction:
Balance the following redox reaction in acidic solution using the half reactions method. CuS (s) + NO3(aq) - Cu² (aq) +S(s) + NO(g) 3CUS (s) + 8H+ (aq) + 2NO3- (aq) →>3Cu^2+ +3S (s) + 2NO (g) + 4H20 (1) Your Answer: 3 CuS (s) +8H (aq) + 2NO3(aq) 3 Cu²+ 3S (s) + 2NO(g) + 4H₂0 (1) -
Balance the following redox reaction in acidic solution. Fe 3+ Fe (aq)+I0,(aq) → "(aq)+I,(s) Fe (ag) + 10, (aq) Fe (ag) + 1, ()
Write balanced half-reactions for the following redox reaction: 12Fe3+(aq)+C2H5OH(l)+12OH−(aq)→ 12Fe2+(aq)+2CO2(g)+9H2O(l)
Balance the following redox reaction in acidic solution using the half reactions method. CuS (s) + NO3 (aq) - → Cu²+ (aq) + S (s) + NO(g) 3 Cu2+(aq) + NO(g) + 2 H2O(I)-> 3 Cu+(aq) + NO3-(aq) + 4 H+(aq) Your Answer: 3 Cu2+ (aq)+ NO (g) + 2 H2 O(1) → 3 Cu* (aq) + NO3 (aq) + 4H†(aq) Attempt: 5 (saved a minute ago) SAVE RESPONSE There is an issue with the chemical species in your reaction. Double check that you have the chemical formulas correct for each compound and that you have input the state correctly. Proper states include (s), (I), (g), and (aq). Anything other than that is incorrect. Specifically, you should look at the reactants.
Complete and balance the following redox reaction in basic solution. Be sure to include the proper phases for all species within the reaction. MnO₄⁻(aq) + C₂O₄²⁻(aq) → MnO₂(s) + CO₂(g)
Balance the following skeletal reaction in acidic solution. Be sure to include “1” in the blank if the coefficient is 1. Ag+(aq) +PbO(s) → PbO2(s) + Ag(s)
In the following redox equation, choose the correct oxidation half equation: 6 103 (aq) + Br (aq) → Br2 (1) + IBr(s) O 103 (aq) + 4 e + IBr(s) Br2 (1) +2e +Br" (aq) 2Br" (aq) + Br2 + 2e (1)
Please don't give handwritten answers is the strongest oxidising agent under standard conditions? Ag+(aq) H2(g) H+(aq) Cl2(g) Al+3(aq)