First, assign oxidation numbers for each atom in the balanced chemical equation below. You'll find it easiest to fill the blanks in left to right since once there is an oxidation number typed in the blank it will be much closer to appearing over the appropriate elemental symbol. Blank 1 Blank 2Blank 3 12Blank 13 Blank 4Blank 5Blank 6 Blank 14Blank 15Blank 16 KMnO4(aq) + KCIO₂(aq) + H₂O(l) → 4 MnO₂(s) + 3 KCIO4(aq) + 4 KOH(aq) Now, identify each of the following • What underwent reduction? Blank 17 Blank 7Blank 8 • What gained electrons? Blank 18 • What got oxidized? Blank 19 • What is the oxidizing agent? Blank 20 • What is the reducer? Blank 21 What lost electrons? Blank 22 Blank 9Blank 10 Blank 11Blank

First, assign oxidation numbers for each atom in the balanced chemical equation below. You'll find it easiest to fill the blanks in left to right since once there is an oxidation number typed in the blank it will be much closer to appearing over the appropriate elemental symbol. Blank 1 Blank 2Blank 3 12Blank 13 Blank 4Blank 5Blank 6 Blank 14Blank 15Blank 16 KMnO4(aq) + KCIO₂(aq) + H₂O(l) → 4 MnO₂(s) + 3 KCIO4(aq) + 4 KOH(aq) Now, identify each of the following • What underwent reduction? Blank 17 Blank 7Blank 8 • What gained electrons? Blank 18 • What got oxidized? Blank 19 • What is the oxidizing agent? Blank 20 • What is the reducer? Blank 21 What lost electrons? Blank 22 Blank 9Blank 10 Blank 11Blank

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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Decide whether each chemical reaction in the table below is an oxidation-reduction ("redox") reaction. If the reaction is a redox reaction, write down the formula of the reducing agent and the formula of the oxidizing agent. S₂ (s) + 4Pb (s) 4PbS₂ (s) 70₂(g) + 2CH₂CH₂(g) → 4CO₂(g) + 611₂0 (g) 3 HSO (aq) + OH¯(aq) → SO² (aq) + H₂0 (1) redox reaction? yes reducing agent: oxidizing 0 agent: redox reaction? yes reducing agent: oxidizing agent: 0 redox reaction? yes reducing agent: oxidizing □ agent: no no no X Ś
Specify which of the following are oxidation-reduction reactions, and if it is, identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced. If it is not, select No and leave the following boxes blank. Express your answers as chemical formulas. Omit states-of-matter. a. CH4 (9) + H2 O(g) → CO(9) + 3H2 (9) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced Yes v b. 2AGNO3 (ag) + Zn(s) → Zn(NO3)2 (aq) + 2Ag(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced No v
Write the net ionic equation for the following molecular equation. Cr2(SO4)3(aq) + 2(NH4)3PO4(aq) 2CrPO4(s) + 3(NH4)2SO4(aq)
Cobalt(II) chloride solution reacts with sodium hydroxide solution. Identity the spectator ion(s). Note: you may choose more than one answer. O Co2+ Na OH
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Fe(s) + CuSO4(aq) and KCL(aq) + AgNO3(aq) For each one write total and net ionic equations.
Be sure to specify states such as (aq) or (s).If a box is not needed leave it blank.If no reaction occurs leave all boxes blank and click on "Submit". Write the net ionic equation for any precipitation reaction that may be predicted when aqueous solutions of barium hydroxide and calcium nitrate are combined. + + + +
Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank. If no reaction occurs leave all boxes blank and click on "Submit". Use H3O* for hydronium ion. Write a net ionic equation for the reaction that occurs when excess nitric acid (aq) and copper(II) carbonate are combined. + + +
1.) Get two medium test tubes. Into one, place about 2 mL of a solution of sodium carbonate. Into the other add about 2 mL of nickel(II) chloride solution. Note the appearances of the two solutions and then mix them together noting any changes that have taken place. Change(s) that took place when the solutions were mixed: Balanced chemical equation: Balanced ionic equation Balanced net ionic equation:
For the following reaction, what happens to the oxidation state of Cl ? 2 ClO2 (g) + 2 I- (aq) ® 2 ClO2 -1 (aq) + I2(s) It does not change It changes from +4 to +5 It changes from -1 to -2 It changes from +4 to +3