Homework Answers
Ans 34 :
To balance the redox reactions, we start by writing the oxidation and reduction half reactions seperately. Then we balance all atoms other than hydrogen and oxygen .
Then oxygen and hydrogen is balanced by adding water molecules and protons respectively.
Charges are balanced by adding electrons.
Half reactions are added and simplified to get the balanced redox reactions as :
2PbO2 + 4H+ = 2Pb2+ + O2 + 2H2O
2Fe2+ + MnO2 + 4H+ = 2Fe3+ + Mn2+ + 2H2O
As2S3 + 5NO3- + 3H2O = 2HAsO42- + 3So + 5NO2- + 4H+
10CH2O + 8NO3- + 3H+= 4N2 + 5HCO3- + 5CO2 + 9H2O
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pore water's corespunucu 34. Balance the following oxidation-reduction reactions: PbO2 (s) → Pb2+ + O2 Fe2+...
2) Depict the half reactions for (2 pt each) Fe2+ oxidation for Fe203 MnO2 reduction to...
2) Depict the half reactions for (2 pt each) Fe2+ oxidation for Fe203 MnO2 reduction to Mn2+ C6H12O6 oxidation to CO2 HS oxidation to Sº UO2 oxidation to UO22+
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...
Please use the half-reaction method! 1. Balance the following redox reactions, using the rules on p....
Please use the half-reaction method!
1. Balance the following redox reactions, using the rules on p. 97 or the half-reaction method, whichever makes more sense to you. a. PbO2() → Pb2+ + O2 b. FeS2(pyrite) + NO3 → N2(g) + FeOOH goethite) + SO42-
7.14 Identify each of the following as an oxidation or a reduction: A. O2(g)+4 e--202-(aq) Oxidation...
7.14 Identify each of the following as an oxidation or a reduction: A. O2(g)+4 e--202-(aq) Oxidation B. Ag(s) Ag+(aq)+e- reduction C. Fe3+(aq)+e-Fe2+(aq) reduction D. 2Br-(aq) →Br2(1)+2 e- oxidation
(10 pts.) (10 pts.) (10 pts.) (10 pts.) 2. Balance the following redox reactions. In all...
(10 pts.) (10 pts.) (10 pts.) (10 pts.) 2. Balance the following redox reactions. In all cases, identify the oxidation states of elements, write the half-reactions and then combine the half-reactions to write the whole reaction. (a) PbO2) - Pb2+ + 0, (b) Fe2+ + MnO213) - Fe2+ + Mn2 (C) CH0(aq) + NO; + HCO; + N2 + CO2(g) 3. Soils in the rice paddies of Mekong delta have been continuously submerged and used for growing rice. These soils...
Balancing Oxidation–Reduction Reactions (Section)Complete and balance the following equations, and identify the oxidizing and reducing agents:(a)...
Balancing Oxidation–Reduction Reactions (Section)Complete and balance the following equations, and identify the oxidizing and reducing agents:(a) Cr2O72-(aq) + I-(aq)→Cr3+(aq) + IO3-(aq) (acidic solution)(b) MnO4-(aq) + CH3OH(aq) →Mn2+(aq) +HCO2H(aq) (acidic solution)(c) I2(s) + OCl-(aq)→IO3-(aq) + Cl-(aq) (acidic solution)(d) As2O3(s) + NO3-(aq)→H3AsO4(aq) + N2O3(aq) (acidic solution)(e) MnO4-(aq) + Br-(aq)→MnO2(s) + BrO3-(aq) (basic solution)(f) Pb(OH)42-(aq) + ClO-(aq)→PbO2(s) + Cl-(aq) (basic solution)
RODOX EXAMINATION An oxidation-reduction reaction involves the (1) sharing of electrons &n
RODOX EXAMINATION An oxidation-reduction reaction involves the (1) sharing of electrons (3) transfer of electrons (2) sharing of protons (4) transfer of protons In this reaction, CO→ 2 CO + O2 the oxidation number of carbon changes from: (1) 0 to +4 (3) +3 to 0 (2) +2 to +4 (4) +4 to +2 Which balanced equation represents a redox reaction? AgNO3 (aq) +NaCl (aq) →AgCl (s) +NaNO3 (aq) H2CO3 (aq)...
(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...
Find the best reducing agent from Cu+, Ag+ F2 and Fe3+ #1. In the reduction table...
Find the best reducing agent from Cu+, Ag+ F2 and Fe3+
#1. In the reduction table i can see several repeated values of
Fe3+ one is equal to 0.77v and the second one is equal to -0.036v
so, which one do I choose? Please explain.
#2.If I'm asked to find the best oxidation agent, from the
values already provided (Cu+, Ag+ F2 and Fe3+) which one would it
be? and how would I decide from repeated values, like in #1,...
Use the galvanic cell notation to describe the Daniell cell. (4 marks) Using the reduction potential...
Use the galvanic cell notation to describe the Daniell cell. (4 marks) Using the reduction potential table calculate Eº for the Daniel cell. 12 marks) Calculate the equilibrium constant K for the reaction Cu2+ + Zn → Cu + Zn²+, at 25 °C. (4 marks) Standard Potentials at 25°C Half Reaction Potential Potential +2.87 V 0.000 V +2.07 V -0.04 V +2.05 V -0.13 V -1.69 V -0.14 V +1.69 V -0.23 V +1.67 V -0.26 V +1.63 v -0.28...
2) Depict the half reactions for (2 pt each) Fe2+ oxidation for Fe203 MnO2 reduction to Mn2+ C6H12O6 oxidation to CO2 HS oxidation to Sº UO2 oxidation to UO22+
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...
Please use the half-reaction method!
1. Balance the following redox reactions, using the rules on p. 97 or the half-reaction method, whichever makes more sense to you. a. PbO2() → Pb2+ + O2 b. FeS2(pyrite) + NO3 → N2(g) + FeOOH goethite) + SO42-
7.14 Identify each of the following as an oxidation or a reduction: A. O2(g)+4 e--202-(aq) Oxidation B. Ag(s) Ag+(aq)+e- reduction C. Fe3+(aq)+e-Fe2+(aq) reduction D. 2Br-(aq) →Br2(1)+2 e- oxidation
(10 pts.) (10 pts.) (10 pts.) (10 pts.) 2. Balance the following redox reactions. In all cases, identify the oxidation states of elements, write the half-reactions and then combine the half-reactions to write the whole reaction. (a) PbO2) - Pb2+ + 0, (b) Fe2+ + MnO213) - Fe2+ + Mn2 (C) CH0(aq) + NO; + HCO; + N2 + CO2(g) 3. Soils in the rice paddies of Mekong delta have been continuously submerged and used for growing rice. These soils...
(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...
Find the best reducing agent from Cu+, Ag+ F2 and Fe3+
#1. In the reduction table i can see several repeated values of
Fe3+ one is equal to 0.77v and the second one is equal to -0.036v
so, which one do I choose? Please explain.
#2.If I'm asked to find the best oxidation agent, from the
values already provided (Cu+, Ag+ F2 and Fe3+) which one would it
be? and how would I decide from repeated values, like in #1,...
Use the galvanic cell notation to describe the Daniell cell. (4 marks) Using the reduction potential table calculate Eº for the Daniel cell. 12 marks) Calculate the equilibrium constant K for the reaction Cu2+ + Zn → Cu + Zn²+, at 25 °C. (4 marks) Standard Potentials at 25°C Half Reaction Potential Potential +2.87 V 0.000 V +2.07 V -0.04 V +2.05 V -0.13 V -1.69 V -0.14 V +1.69 V -0.23 V +1.67 V -0.26 V +1.63 v -0.28...
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