**EXPERIMENT 5: REDOX REACTIONS****Copy these tables into your laboratory notebook:**---**System:** | | #1: Cu and HNO₃ | #2: Cu and HCl ||---|---|---|| **Prediction:** Should you expect H₂(g) to be evolved? Why or why not? | | || **What gas(es) might be emitted if the nitrate ion reacts?** | | || **Observations:** | | (Shaded area indicating no entry needed) || **Net ionic equation for the reaction, if any:** | | |---**System 3: NaHSO₃ and KMnO₄****Prediction**1. Is the HSO₃⁻ ion a possible oxidizing agent? _______ - If yes, to what species could it change? __________2. Is it a possible reducing agent? _______ - If yes, to what species could it change? __________3. Is the MnO₄⁻ ion a possible oxidizing agent? _______ - If yes, list the species to which it could change, their colors and conditions that favor each change: ___________________________________________________Why is the MnO₄⁻ ion not a possible reducing agent?______________________________________________________________________________________________________ **Net Ionic Equations****[3A]** ___MnO₄⁻(aq) + ___HSO₃⁻(aq) + _____ → _____ + _____ + _____**[3B]** ___MnO₄⁻(aq) + ___SO₃²⁻(aq) + _____ → _____ + _____ + _____**[3C]** ___MnO₄⁻(aq) + ___SO₃²⁻(aq) + _____ → _____ + _____ + _____---**System 4 KI and FeCl₃****Prediction**What possible redox role(s) can the iodide ion assume? ________________To what species could it be converted? ________________________What possible redox roles(s) can the Fe³⁺ ion assume? _________________To what species could it be converted? _____________________**Observations**________________________________________________________________**Net Ionic Equation**________________________________________________________________

Since you have asked multiple questions, we will answer the first one for you To get the remaining question solved, please repost the complete question which you want us to solve.1) In the reaction involving copper and nitric acid as reactants, H2 gas is not evolved. This is because nitric acid is a strong oxidizing agent which oxidizes H2 to H2O and itself gets reduced to nitrogen oxides. When the nitrate ion reacts, redox reaction takes place in which copper is oxidized to Cu2+ forming copper nitrate, hydrogen oxidized to water and nitrate ion itself reduces to any of the nitrogen oxide gases- N2O, NO, NO2. For example: Cu (s)+4HNO3 (aq)→Cu(NO3)2 (aq) +2NO2 (g)+2H2O (l) Observation- the solution turns blue as a result of oxidation of Cu to Cu2+. Net ionic equation: Cu (s)+4H++4NO3- (aq)→Cu2+(aq)+2NO3- (aq) +2NO2 (g)+2H2O (l)≡Cu (s)+4H++2NO3- (aq)→Cu2+(aq)+2NO2 (g)+2H2O (l)2) No reaction takes place between copper and hydrochloric acid since copper is below hydrogen in the activity series and thus, copper will not displace hydrogen from hydrochloric acid and thus, hydrogen gas is not evolved. Observation- No change observed. Net ionic equation: Cu(s)+HCl(aq)→No Reaction

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System: Prediction: Should you expect H₂(g) to be evolved? Why or why not? What gas(es) might be emitted if the nitrate ion reacts? Observations: Net ionic equation for the reaction, if any #1: Cu and HNO3 System 3: NaHSO3 and KMnO4 Prediction Is the HSO; ion a possible oxidizing agent? If yes, to what species could it change? Is it a possible reducing agent? If yes, to what species could it change? # 2: Cu and HCI Is the MnO4 ion a possible oxidizing agent? If yes, list the species to which it could change, their colors and conditions that favor each change: Why is the MnO4 ion not a possible reducing agent?

System: Prediction: Should you expect H₂(g) to be evolved? Why or why not? What gas(es) might be emitted if the nitrate ion reacts? Observations: Net ionic equation for the reaction, if any #1: Cu and HNO3 System 3: NaHSO3 and KMnO4 Prediction Is the HSO; ion a possible oxidizing agent? If yes, to what species could it change? Is it a possible reducing agent? If yes, to what species could it change? # 2: Cu and HCI Is the MnO4 ion a possible oxidizing agent? If yes, list the species to which it could change, their colors and conditions that favor each change: Why is the MnO4 ion not a possible 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

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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import from another browser. Import favorites [Review Topics] Although there are a number of magnesium-containing minerals, the commercial source of this metal is seawater. Treatment of seawater with Ca(OH)2 gives insoluble Mg(OH)2- This reacts with HCl to produce MgCl,, which is dried, and the metal is [References] obtained by electrolysis of the molten salt. (The density of seawater is 1.025 g/cm and the concentration of Mg* in seawater is 0.052 mol/L.) 2+ Calculate the mass of Mg that could be obtained by the process described above from 8.0 L of seawater. Mass = To prepare 290. kg of Mg, what volume of seawater would be needed? Volume Retry Entire Group 4 more group attempts remaining Submit Answwer 6:42 PM A6 40 3/21/2020 FLP 80
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