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POST-LABORATORY QUESTIONS Procedure: Balance the redox reactions given below. Show your work on a separate sheet...
not sure if i did either of these right and i need help solving the rest...
not sure if i did either of these right and i need help
solving the rest of it. thanks
error in your experiment. POST-LABORATORY QUESTIONS Procedure: Balance the redox reactions given below. Show your work on a separate sheet of paper. Write the balanced oxidation and reduction half reactions; also identify the oxidizing agent and the reducing agent. All reactions are to be balanced in acidie media, except when OH is shown. (0) Cu + 2 NO, + 4 H...
i need help with these redox reactions H NO; + Re s or + H₂O Fes:...
i need help with these redox reactions
H NO; + Re s or + H₂O Fes: NO, pyrite) Oxidation Hall Reaction: Reduction Half Reaction: Oxidizing agent Reducing agent Mn? + HO; + OH MnO + H2O Oxidation Half Reaction: Reduction Hall Reaction: Oxidizing agent: Reducing agent _MnO + NO + H2O → MnO: + NO + OH- Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent 0 Clz + OH - CH + CIO + H:0 Oxidation Half Reaction:...
Balance the redox reaction given 7. H → NO2+ Fe + SO4 + H2O FeS2 +...
Balance the redox reaction given
7. H → NO2+ Fe + SO4 + H2O FeS2 + NO3 + (pyrite) Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent
Experiment 14 Report Sheet Oxidation-Reduction Reactions Dato Lab Sec.-_ Name Desk No. A. Oxidation-Reduction Reactions I...
Experiment 14 Report Sheet Oxidation-Reduction Reactions Dato Lab Sec.-_ Name Desk No. A. Oxidation-Reduction Reactions I . ①Oxidation of Magnesium. Write a description of the reaction, what did the litmus tests reveal? Write a balanced equation for the oxidation of magnesium in air. Box] the oxidizing agent in the equation 2. ②Oxidation of Copper. Describe your observations of each lest tube. Comment on the relative oxidizing strengths of the three acids in the test tubes. eactions. On a separate sheet...
Write the half-reactions and the net ionic equations for these complete redox reactions 4 2NaCl (aq) + Br: (I) Cl:...
Write the half-reactions and the net ionic equations for these complete redox reactions 4 2NaCl (aq) + Br: (I) Cl: (g)2NaBr (aq) a) Oxidation half-reaction: Reduction half-reaction: CrCls (aq)+ Au (s) AuCl3(aq) Cr (s) - b) Oxidation half-reaction: Reduction half-reaction: Identify the oxidizing agent and the reducing agent in these complete redox reactions: 5. 5SO2-2Mn2+ 5so +3H2O a) 2MnO, +6H A) MnO B) So2 C) Mn2 D) SO E) H Oxidizing agent: b) 5Fe2 (aq) + MnO4 (ag) +8H'(aq)-5Fe (ag)+...
Be sure to answer all parts. For the complete redox reactions given here, write the half-reactions...
Be sure to answer all parts. For the complete redox reactions given here, write the half-reactions and identify the oxidizing and reducing agents. Make sure your answer has the simplest coefficients Part 1 out of 4 (a) 4Fe+3o2- 2Fe203 Select the oxidizing agent: 0 02 Fe Fe+ o2- Oxidation: Fe Fe +3 Reduction: 02+420
Identify if the following reactions are redox in nature or not. Then identify the I) oxidation,...
Identify if the following reactions are redox in nature or not. Then identify the I) oxidation, reduction, oxidizing agent and reducing agent 3 2 Fe:O3 (s)+CO (g) -> FeO (s) + CO (g) Ca (s) + H20 ()-> Ca(OH)2 (aq)+H2 (g)
The following is a redox reaction, which takes place in acidic solution: Fe (s) + HC1...
The following is a redox reaction, which takes place in acidic solution: Fe (s) + HC1 (aq) = HFeCl4 (aq) + H2 (g) The oxidation half-reaction is: The reduction half-reaction is: The oxidizing agent is the reducing agent is: The total number of electrons transferred in the balanced redox reaction is Can you please explain how you get everything please! I have the answers i just don't understand how to get there
Data Activity 1 Data Table 1 Fe2+ (FeSO) No. of Reactions Metal Tested Mg2+ (MgSO4) Mg(s)...
Data Activity 1 Data Table 1 Fe2+ (FeSO) No. of Reactions Metal Tested Mg2+ (MgSO4) Mg(s) Fe(s) Cu(s) Cu2+ (Cusos) 3 T 3 toleast most 1. Use the number of reactions in Data Table 1 to list the metals copper, iron, reactive and magnesium in order from most reactive to least reactive. 2. Summarize the redox reactions that you observed in this investigation. List the reactions in descending order of activity, referring to Data Table 1. For each reaction in...
Redox Equations Which of the following reactions are redox reactions? Identify the substance oxidized, the substance...
Redox Equations Which of the following reactions are redox reactions? Identify the substance oxidized, the substance reduced, the oxidizing agent, the reducing agent. 1.2 Mg(s) + O2(g) → 2 MgO (s) 2. H SO. (aq) + Al(OH) (aq) → Al(SO.) (aq) + H,O (1) 3. 2 Na (s) + H2O (1) ► 2 NaOH(aq) + H2(g) 4. Cao (s) + CO2(g) → Caco, (s) 5. AgNO, (aq) + NaCl (aq) ► AgCl(s) + NaNO, (aq) Identify the substance oxidized, the...
not sure if i did either of these right and i need help
solving the rest of it. thanks
error in your experiment. POST-LABORATORY QUESTIONS Procedure: Balance the redox reactions given below. Show your work on a separate sheet of paper. Write the balanced oxidation and reduction half reactions; also identify the oxidizing agent and the reducing agent. All reactions are to be balanced in acidie media, except when OH is shown. (0) Cu + 2 NO, + 4 H...
i need help with these redox reactions
H NO; + Re s or + H₂O Fes: NO, pyrite) Oxidation Hall Reaction: Reduction Half Reaction: Oxidizing agent Reducing agent Mn? + HO; + OH MnO + H2O Oxidation Half Reaction: Reduction Hall Reaction: Oxidizing agent: Reducing agent _MnO + NO + H2O → MnO: + NO + OH- Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent 0 Clz + OH - CH + CIO + H:0 Oxidation Half Reaction:...
Balance the redox reaction given
7. H → NO2+ Fe + SO4 + H2O FeS2 + NO3 + (pyrite) Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent
Experiment 14 Report Sheet Oxidation-Reduction Reactions Dato Lab Sec.-_ Name Desk No. A. Oxidation-Reduction Reactions I . ①Oxidation of Magnesium. Write a description of the reaction, what did the litmus tests reveal? Write a balanced equation for the oxidation of magnesium in air. Box] the oxidizing agent in the equation 2. ②Oxidation of Copper. Describe your observations of each lest tube. Comment on the relative oxidizing strengths of the three acids in the test tubes. eactions. On a separate sheet...
Write the half-reactions and the net ionic equations for these complete redox reactions 4 2NaCl (aq) + Br: (I) Cl: (g)2NaBr (aq) a) Oxidation half-reaction: Reduction half-reaction: CrCls (aq)+ Au (s) AuCl3(aq) Cr (s) - b) Oxidation half-reaction: Reduction half-reaction: Identify the oxidizing agent and the reducing agent in these complete redox reactions: 5. 5SO2-2Mn2+ 5so +3H2O a) 2MnO, +6H A) MnO B) So2 C) Mn2 D) SO E) H Oxidizing agent: b) 5Fe2 (aq) + MnO4 (ag) +8H'(aq)-5Fe (ag)+...
Be sure to answer all parts. For the complete redox reactions given here, write the half-reactions and identify the oxidizing and reducing agents. Make sure your answer has the simplest coefficients Part 1 out of 4 (a) 4Fe+3o2- 2Fe203 Select the oxidizing agent: 0 02 Fe Fe+ o2- Oxidation: Fe Fe +3 Reduction: 02+420
Identify if the following reactions are redox in nature or not. Then identify the I) oxidation, reduction, oxidizing agent and reducing agent 3 2 Fe:O3 (s)+CO (g) -> FeO (s) + CO (g) Ca (s) + H20 ()-> Ca(OH)2 (aq)+H2 (g)
Data Activity 1 Data Table 1 Fe2+ (FeSO) No. of Reactions Metal Tested Mg2+ (MgSO4) Mg(s) Fe(s) Cu(s) Cu2+ (Cusos) 3 T 3 toleast most 1. Use the number of reactions in Data Table 1 to list the metals copper, iron, reactive and magnesium in order from most reactive to least reactive. 2. Summarize the redox reactions that you observed in this investigation. List the reactions in descending order of activity, referring to Data Table 1. For each reaction in...
Redox Equations Which of the following reactions are redox reactions? Identify the substance oxidized, the substance reduced, the oxidizing agent, the reducing agent. 1.2 Mg(s) + O2(g) → 2 MgO (s) 2. H SO. (aq) + Al(OH) (aq) → Al(SO.) (aq) + H,O (1) 3. 2 Na (s) + H2O (1) ► 2 NaOH(aq) + H2(g) 4. Cao (s) + CO2(g) → Caco, (s) 5. AgNO, (aq) + NaCl (aq) ► AgCl(s) + NaNO, (aq) Identify the substance oxidized, the...
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