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Which of the following reactions are redox reactions? In those that are, identify the oxidation and...
All the following are oxidation–reduction reactions except: a.) H2(g) + F2(g) → 2HF(g). b.) Ca(s) +...
All the following are oxidation–reduction reactions except: a.) H2(g) + F2(g) → 2HF(g). b.) Ca(s) + H2(g) → CaH2(s). c.) 2K(s) + 2H2O(l) → 2KOH(aq) + H2(g). d.) 6Li(s) + N2(g) → 2Li3N(s). e.) Mg3N2(s) + 6H2O(l) → 3Mg(OH)2(s) + 2NH3(g).
Which of the following are redox reactions? Explain your answer on the basis of changes in...
Which of the following are redox reactions? Explain your answer on the basis of changes in oxidation number 1. CuSO4 + 2NaOH → Cu(OH) 2 + Na 2504 2. 2A1 + 3MgSO4 → 3Mg + Al 2(SO4)3 3. 2(NH4)3PO4 + 3Ba(NO3)2 - Ba 3(PO4)2 + 6NH4NO3 4.2HNO3 + 3H3ASO3 2NO + 3H 3ASO4+H2O
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)
Chemical equations of reduction–oxidation (redox) reactions can be quite nontrivial to balance. To do so, you...
Chemical equations of reduction–oxidation (redox) reactions can be quite nontrivial to balance. To do so, you begin with balancing the number of electrons some particles lose in oxidation and other particles gain in reduction. Consider a reaction between potassium permanganateKMnO4 andhydrochloricacidHCl(aq), which can be used in a lab to produce chlorine gas Cl2. In this reaction, a MnO− 4 ion is reduced to a Mn2+ ion by getting electrons from Cl− and losing its oxygen atoms to bind with H+...
Balance the following Redox Equations in Basic Mediums. Redox Reactions in Basic Solution 1. Al(s) + ...
Balance the following Redox Equations in Basic Mediums. Redox Reactions in Basic Solution 1. Al(s) + MnO4¯ (aq) ¾® MnO2(s) + Al(OH)4¯ (aq) 2. NO2¯ (aq) + Al(s) ¾® NH3(aq) + AlO2¯ (aq) 3. Cr(s) + CrO42-(aq) ¾® Cr(OH)3(s) Note: Cr(OH)3 is found in BOTH half reactions! 4. Cl2(aq) + Br2(l) ¾® OBr¯ (aq) + Cl¯ (aq) 5. S8(aq) + MnO4¯ (aq) ¾® SO42-(aq) + MnO2(s)
Balance the following oxidation-reduction equations. The reactions occur in acidic solution. (Use the lowest possible coefficients....
Balance the following oxidation-reduction equations. The reactions occur in acidic solution. (Use the lowest possible coefficients. Omit states of matter. Add H20 or H to any side of the reaction if it is needed.) a. Pb + Bi0,- + PbO2+ BiS+ Pb + BiO3 + PbO2 + Bi9+ + b. Cr,0,? + Fe2+ + Cr+ + Fe3+ | Cr₂O₂ ² + | Fe²+ + + Fel- c. MnO, +1“ + Mn2+ + Cl2 MnO2 + Cl + Mn + Cl2...
(10 pts) Balance the following redox reactions by first separating the oxidation and reduction half-reactions. a....
(10 pts) Balance the following redox reactions by first separating the oxidation and reduction half-reactions. a. Cut (aq) + Fe (s) Fe3+ (aq) + Cu(s) b. Cu(s) + HNO3 (aq) Cu2+ (aq) + NO (g) (basic solution) c. NH(aq) + O2(g) → N03 (aq) + H2O(l) (acidic solution) d. Cd(s) + NiO(OH)(s) + Ca(OH)2(s) + Ni(OH)2(s) (Nicad battery) e. The oxidation of iodide ion (1) by permanganate ion (MnO4) in basic solution to yield molecular iodine (12) and manganese(IV) oxide...
Name Chapter 4 Classwork Part 2 Chemical Reactions 1. In the following redox reaction, identify the oxidation and r...
Name Chapter 4 Classwork Part 2 Chemical Reactions 1. In the following redox reaction, identify the oxidation and reduction half-reactions. Which element is oxidized and which element is reduced? 4NH,+3Ca(CI)2N2+6H2O+3CaCl 2. The oxidation number of N in NaNO, is 3. The oxidation number of S in K2SO, is 4. The oxidation number of Mn in KMnO4 is 5. The oxidation number of Fe in KaFe(CN)s is 6. The oxidation number of Cr in CrO is 7. The oxidation number of...
balance the following redox reactions in acidic solution by the half reaction method. Indicate which half...
balance the following redox reactions in acidic solution by the
half reaction method. Indicate which half reaction is for oxidation
and which for reduction.
b) Cr2O72- (aq) + CH(aq) > Cr*(aq) + Cl2(g) c) Au(s) + HNO3(aq) + HCl(aq) --> AuCl4- (aq) + NO(g) d) 103-(aq) + (aq) --> 13-(aq)
Separate the following redox reactions into half-reactions, and label each half-reaction as oxidation or reduction. Part...
Separate the following redox reactions into half-reactions, and label each half-reaction as oxidation or reduction. Part A Oxidation half-reaction for 2Li(s)+2H+(aq)→2Li+(aq)+H2(g). Express your answer as a chemical equation. Identify all of the phases in your answer. Part B Oxidation half-reaction for 2Ag+(aq)+Be(s)→Be2+(aq)+2Ag(s). Express your answer as a chemical equation. Identify all of the phases in your answer.
Which of the following are redox reactions? Explain your answer on the basis of changes in oxidation number 1. CuSO4 + 2NaOH → Cu(OH) 2 + Na 2504 2. 2A1 + 3MgSO4 → 3Mg + Al 2(SO4)3 3. 2(NH4)3PO4 + 3Ba(NO3)2 - Ba 3(PO4)2 + 6NH4NO3 4.2HNO3 + 3H3ASO3 2NO + 3H 3ASO4+H2O
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)
Balance the following oxidation-reduction equations. The reactions occur in acidic solution. (Use the lowest possible coefficients. Omit states of matter. Add H20 or H to any side of the reaction if it is needed.) a. Pb + Bi0,- + PbO2+ BiS+ Pb + BiO3 + PbO2 + Bi9+ + b. Cr,0,? + Fe2+ + Cr+ + Fe3+ | Cr₂O₂ ² + | Fe²+ + + Fel- c. MnO, +1“ + Mn2+ + Cl2 MnO2 + Cl + Mn + Cl2...
(10 pts) Balance the following redox reactions by first separating the oxidation and reduction half-reactions. a. Cut (aq) + Fe (s) Fe3+ (aq) + Cu(s) b. Cu(s) + HNO3 (aq) Cu2+ (aq) + NO (g) (basic solution) c. NH(aq) + O2(g) → N03 (aq) + H2O(l) (acidic solution) d. Cd(s) + NiO(OH)(s) + Ca(OH)2(s) + Ni(OH)2(s) (Nicad battery) e. The oxidation of iodide ion (1) by permanganate ion (MnO4) in basic solution to yield molecular iodine (12) and manganese(IV) oxide...
Name Chapter 4 Classwork Part 2 Chemical Reactions 1. In the following redox reaction, identify the oxidation and reduction half-reactions. Which element is oxidized and which element is reduced? 4NH,+3Ca(CI)2N2+6H2O+3CaCl 2. The oxidation number of N in NaNO, is 3. The oxidation number of S in K2SO, is 4. The oxidation number of Mn in KMnO4 is 5. The oxidation number of Fe in KaFe(CN)s is 6. The oxidation number of Cr in CrO is 7. The oxidation number of...
balance the following redox reactions in acidic solution by the
half reaction method. Indicate which half reaction is for oxidation
and which for reduction.
b) Cr2O72- (aq) + CH(aq) > Cr*(aq) + Cl2(g) c) Au(s) + HNO3(aq) + HCl(aq) --> AuCl4- (aq) + NO(g) d) 103-(aq) + (aq) --> 13-(aq)
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