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3. Where appropriate, construct half-equations for the following reactions and use them to balance the full...
2. For the formation of each of the following ionic compounds from their elements, write an...
2. For the formation of each of the following ionic compounds from their elements, write an overall equation showing the formation of the compound. Then write two half- equations to identify the REDOX process. (a) calcium sulfide (b) aluminum bromide (c) aluminum oxide 3. Where appropriate, construct half-equations for the following reactions and use them to balance the full equations. † † (a) 10;' ++ (b) 12 + S2032 (c) Br2 + KI (d) MnO 2 + H (e) Cro.2...
Balance the following redox reactions by balancing the half reactions and then combine the half reactions...
Balance the following redox reactions by balancing the half reactions and then combine the half reactions to get the overall balanced redox reaction with the lowest possible whole number coefficients. 1. Consider the following unbalanced redox reaction: MnO2(s) + BrO3−(aq) → MnO4−(aq) + Br−(aq) (a) Balance the corresponding half reactions in acidic conditions using the lowest possible whole number coefficients. (Enter coefficients for one and zero. Blanks will be marked incorrect.) MnO2(s) + H2O(l) + OH−(aq) + H+(aq) + e− → MnO4−(aq) + H2O(l) + OH−(aq) + H+(aq)...
Balance the following equations. (Use the lowest possible whole-number coefficients. These may be zero.) Balance the...
Balance the following
equations. (Use the lowest possible whole-number coefficients.
These may be zero.)
Balance the following equations. (Use the lowest possible whole-number coefficients. These may be zero.) (a) Cr2022(aq) + I (aq) = Cr3+ (aq) + 103 (aq) 1 Cr2O72- + 1 1 + 8 H+ + 1 X H20 = 2 Cr3+ + 1 103 + 1 X H+ + 4 H2O (b) CIO3-aq) + As(s) Æ HCIO(aq) + H3A5O3(aq) 3 CIO3 + 4 As + 3 H...
Balance the following redox equations by the half-reaction method: (a) Mn2+ + H2O2 → MnO2 +...
Balance the following redox equations by the half-reaction method: (a) Mn2+ + H2O2 → MnO2 + H2O (in basic solution) (b) Bi(OH)3 + SnO22− → SnO32− + Bi (in basic solution) (c) Cr2O72− + C2O42− → Cr3+ + CO2 (in acidic solution) (d) ClO3− + Cl− → Cl2 + ClO2 (in acidic solution) (e) Mn2+ + BiO3− → Bi3+ + MnO4− (in acidic solution)
4.102. Balance the following half-reactions by adding the appropriate number of electrons. Which are oxidation half...
4.102. Balance the following half-reactions by adding the appropriate number of electrons. Which are oxidation half reactions and which are reduction half-reactions a. Fe2+ (aq) → Fe3+ (aq) b. Agi() ► Ag(s) + I (ag) c. VO,*(aq) + 2 H+ (aq) → VO2+ (aq) + HOO) d. 1() + 6 H2O(C) – 2 10,- (aq) + 12 H*(aq)
4. Which of these are half reactions (i.e. which will require H20, H', and electrons to balance) and please complete the half reactions? Which are already full RXNs and need only to be balanced i...
4. Which of these are half reactions (i.e. which will require H20, H', and electrons to balance) and please complete the half reactions? Which are already full RXNs and need only to be balanced in terms of moles each (and please balance them)? Which are oxidations and which are reductions? Are any neither oxidations nor reductions C6H1206+ O2 -> CO2 +H2O NH4NO3 NH4 NO3 NH4NO3
4. Which of these are half reactions (i.e. which will require H20, H', and electrons...
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)
1. Provide products for the following reactions. Show appropriate stereochemistry where appropriate. HI H2SO4 CH,OH 1....
1. Provide products for the following reactions. Show appropriate stereochemistry where appropriate. HI H2SO4 CH,OH 1. Hg(OAc),/H,0 2. NaBH4 1. BH; 2. H,Oz/NaOH H/Pd H2SO4/H2O 4. Provide the missing reagents or starting materials in the following reactions. OH Br HO 1. Br2 2, NaNH (excess) 3. H2O
(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...
Fill in the blanks with the appropriate numbers to balance the half reactions and the overall reactions. Note: H,O,...
Fill in the blanks with the appropriate numbers to balance the half reactions and the overall reactions. Note: H,O, OH", H,0 and e" (and CT") are repeated on both sides, obviously some will be 0. 1) MnO, + Cu - MnO, + Cu?" in acidic solution. MnO, + 2 H,0 + OH' + 3 e MnO, + OH,O + 4H+ Oc I Cu + OH,O + OH+ 0 0 - | Cu? + OH,O + OH' + 20 3 Cu...
2. For the formation of each of the following ionic compounds from their elements, write an overall equation showing the formation of the compound. Then write two half- equations to identify the REDOX process. (a) calcium sulfide (b) aluminum bromide (c) aluminum oxide 3. Where appropriate, construct half-equations for the following reactions and use them to balance the full equations. † † (a) 10;' ++ (b) 12 + S2032 (c) Br2 + KI (d) MnO 2 + H (e) Cro.2...
Balance the following
equations. (Use the lowest possible whole-number coefficients.
These may be zero.)
Balance the following equations. (Use the lowest possible whole-number coefficients. These may be zero.) (a) Cr2022(aq) + I (aq) = Cr3+ (aq) + 103 (aq) 1 Cr2O72- + 1 1 + 8 H+ + 1 X H20 = 2 Cr3+ + 1 103 + 1 X H+ + 4 H2O (b) CIO3-aq) + As(s) Æ HCIO(aq) + H3A5O3(aq) 3 CIO3 + 4 As + 3 H...
4.102. Balance the following half-reactions by adding the appropriate number of electrons. Which are oxidation half reactions and which are reduction half-reactions a. Fe2+ (aq) → Fe3+ (aq) b. Agi() ► Ag(s) + I (ag) c. VO,*(aq) + 2 H+ (aq) → VO2+ (aq) + HOO) d. 1() + 6 H2O(C) – 2 10,- (aq) + 12 H*(aq)
4. Which of these are half reactions (i.e. which will require H20, H', and electrons to balance) and please complete the half reactions? Which are already full RXNs and need only to be balanced in terms of moles each (and please balance them)? Which are oxidations and which are reductions? Are any neither oxidations nor reductions C6H1206+ O2 -> CO2 +H2O NH4NO3 NH4 NO3 NH4NO3
4. Which of these are half reactions (i.e. which will require H20, H', and electrons...
1. Provide products for the following reactions. Show appropriate stereochemistry where appropriate. HI H2SO4 CH,OH 1. Hg(OAc),/H,0 2. NaBH4 1. BH; 2. H,Oz/NaOH H/Pd H2SO4/H2O 4. Provide the missing reagents or starting materials in the following reactions. OH Br HO 1. Br2 2, NaNH (excess) 3. H2O
(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...
Fill in the blanks with the appropriate numbers to balance the half reactions and the overall reactions. Note: H,O, OH", H,0 and e" (and CT") are repeated on both sides, obviously some will be 0. 1) MnO, + Cu - MnO, + Cu?" in acidic solution. MnO, + 2 H,0 + OH' + 3 e MnO, + OH,O + 4H+ Oc I Cu + OH,O + OH+ 0 0 - | Cu? + OH,O + OH' + 20 3 Cu...
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