Balancing Redox Equations Using the Oxidation Number Method

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Questions

• How do you balance redox reactions in basic solution?
• How do you balance redox equations by oxidation number method?
• How do you balance redox equations in acidic solutions?
• What is the oxidation number method?
• What are some examples of balancing redox equations using the oxidation number method?
• Why is the oxidation number method useful?
• Is it necessary to break the equation into half reactions in the oxidation number method?
• What is the difference between the oxidation number method and the ion-electron method?
• Can you balance the equation using the oxidation states method MnO2+Al--->Mn+Al2O3?
• How do you balance this redox reaction using the oxidation number method? Fe2+(aq) + MnO4–(aq) --> Fe3+(aq) + Mn2+(aq)
• How do you balance this redox reaction using the oxidation number method? HNO3(aq) + H3AsO3(aq) --> NO(g) + H3AsO4(aq) + H2O(l)
• What is the difference between the oxidation number method and the half-reaction method?
• How do you balance this redox reaction using the oxidation number method? HNO3(aq) + C2H6O(l) + K2Cr2O7(aq) → KNO3(aq) + C2H4O(l) + H2O(l) + Cr(NO3)3(aq)
• How do you balance this redox reaction using the oxidation number method? Al(s) + H2SO4(aq) → Al2(SO4)3(aq) + H2(g)
• How do you balance this redox reaction using the oxidation number method? KClO3(s) → KCl(s)+O2(g)
• Question #91e2a
• Question #51215
• How do you balance this chemical equation? #"KMnO"_4 + "Na"_2"C"_2"O"_4 + "H"_2"SO"_4 → "K"_2"SO"_4 + "Na"_2"SO"_4 + "MnSO"_4 + "CO"_2 + "H"_2"O"#
• How do you balance the acid equation #"MnO"_4^"-" + "H"^"+" + "HSO"_3^"-" → "Mn"^"2+" + "SO"_4^"2-" + "H"_2"O"#?
• Question #33342
• Question #4e8ae
• What are the coefficients in front of NO3-(aq) and Cu(s) when the following redox equation is balanced in an acidic solution: ___ NO3-(aq) + ___ Cu(s) → ___ NO(g) + ___ Cu2+(aq)? A) 2, 6 B) 3, 6 C) 3, 4 D) 2, 3
• Question #79236
• Question #ebe14
• How do you balance the following redox reaction? #"MnO"_4^(-) + "I"^(-) -> "MnO"_2 + "IO"_3^(-)# ?
• Question #de191
• Question #01c4d
• Question #84f03
• Question #6f441
• Question #4b8db
• How to I write half reactions and balance this oxidation-reduction reaction? #S_2O_(8(aq))^(2-) + Cr_((aq))^(3+) -> SO_(4(aq))^(2-) + Cr_2O_(7(aq))^(2-)#
• Question #8d261
• How to balance #Zn + HNO_3 -> Zn(NO_3)_2 + NH_4NO_3 + H_2O#?
• How do you balance the redox reaction? #"KMnO"_4 + "H"_2"O"_2 + "H"_2"SO"_4 -> "MnSO"_4 + "K"_2"SO"_4 + "O"_2 + "H"_2"O"# ?
• Question #92fde
• Question #e32d1
• How does lead sulfide react with oxygen gas to form #PbO#, and #SO_2#?
• Question #2e551
• Question #3d7dc
• Question #1d773
• Question #21c09
• Question #15bad
• How do we represent the oxidation of copper metal to #"cupric ion"#, with accompanying reduction of nitrate ion to #NO(g)#?
• How would you balance the following equation: #"S" + "HNO"_3 -> "H"_2"SO"_4 + "NO"_2 + "H"_2"O"# ?
• Question #c9eb6
• Question #755f2
• Question #86362
• Question #92bc1
• Question #7eb16
• How do we solve a redox equation when BASIC conditions are specified?
• How do you balance #Cu + H_2SO_4 -> CuSO_4 + SO_2 + H_2O# and identify the element oxidized and the oxidizing agent?
• How is #"thiosulfate anion"#, #S_2O_3^(2-)#, oxidized by #"permanganate anion"#, #MnO_4^(-)#?
• How could sulfur be oxidized to #SO_3# by the action of #NO_3^(-)#?
• How do you balance #Al(s) + S(s) -> Al_2S_3(s)#?
• How do you balance #K+B_2O_3 -> K_2O + B#?
• What is the oxidation half reaction for #Fe(s) + 2HCl(aq) -> FeCl_2(aq) + H_2(g)#?
• Question #319b1
• What is the difference between oxidation number and oxidation state?
• How do you balance #CO(g) + I_2O_5(s) -> I_2(s) + CO_2(g)#?
• Can you represent the reduction of dinitrogen pentoxide by dihydrogen gas?
• Balance this redox reaction in acidic media? #"As"_2"O"_3(s) + "NO"_3^(-)(aq) -> "H"_3"AsO"_4(aq) + "N"_2"O"_3(aq)#
• How do you use the half-equation to represent oxidation-reduction reactions?
• How do you balance #SO_3(g) -> SO_2(g) + O_2(g)#?
• What do we call the process when oxygen gas reacts with a SINGLE electron?
• Will methylated spirit dissolve iodine? Will it dissolve sodium chloride or potassium permanganate?
• Upon treatment of a #14.75*g# mass of #MnO_2# with excess #HCl(aq)#, what VOLUME of chlorine gas is generated under standard conditions...?
• For a certain reaction #2A + B rightleftharpoons C + 3D#, #K_(eq) = 4.2 xx 10^3#, which of the following is true?
• Question #cc55e
• Question #f3a1e
• Question #59ff2
• How do represent the oxidation of chloride anion to chlorine in acidic solution?
• In the oxidation of oxalate ion, #C_2O_4^(2-)# to give carbon dioxide by potassium permanganate, #K^(+)MnO_4^(-)#, how do we vizualize the endpoint?
• What is the first step to balance a redox equation using the half-reaction method?
• What is the reduction half-reaction for the unbalanced redox equation #Cr_2O_7^(2-) + NH_4^+ -> Cr_2O_3 + N_2#?
• Question #2fc11
• How is zinc metal oxidized, and nitrate ion reduced to give ammonium ion in aqueous by the action of nitric acid on zinc?
• How do you balance disproportionation redox reactions?
• How do you balance this reaction? #"K"_2"Cr"_2"O"_7(aq) + "H"_2"SO"_4(aq) + "H"_2"S"(aq) -> "Cr"_2("SO"_4)_3(aq) + "H"_2"O"(l) + "S"(s) + "K"_2"SO"_4(aq)#
• Question #d0498
• How do we represent #(i)# represent the reduction of #"chlorate ion"#, #ClO_3^(-)#, to give #ClO_2#?
• When using the half reaction method of balancing redox reactions, what should you do first?
• When balancing a redox reaction, what are you balancing?
• Question #ebe51
• How do you balance #Al+Cl_2->AlCl_3#?
• The change in oxidation state of Mn element in the reaction , 3MnO4²- + 4H+→ MnO2+2MnO4- + 2H2O is? Please help me, thanks.
• Is the reaction of #"lead sulfide"# with #"dioxygen gas"# to give #"lead oxide"#, and #"sulfur dioxide"#, a redox reaction?
• How is pyrophosphate anion, #P_2O_7^(4-)# reduced to elemental phosphorus, with oxidation of hydrogen sulfide to sulphur?
• Question #ddcdf
• Question #a8904
• How do you represent the redox reaction of chlorate ion, #ClO_3^(-)# with #SO_2(g)# to give #Cl^(-)# and #SO_4^(2-)#?
• Question #bfe80
• Question #bb687
• What is the redox equation for the oxidation of potassium chloride to chlorine gas by potassium permanganate in the presence of sulfuric acid?
• How do we represent the oxidation of hydrogen sulfide by nitric acid to give sulfur and #NO(g)#?
• What is the coefficient for #H^+# when the redox equation below is balanced?
• Given that the sulfate(IV) ion, #SO_2^(-2)#, is converted to the sulfate(VI) ion, #SO_4^(-2)#, in the presence of water, deduce the balanced equation for the redox reaction between #Cr_2O_7^(-2)# (aq) and #SO_3^(-2)#?
• Question #ec000
• Question #de72a
• Can you help me balance this equation? As2S3 + K2Cr2O7 + H2SO4 = H3AsO4 + K2SO4 + Cr2(SO4)3 + H2O + SO2
• How do you represent the oxidation of #SO_2(g)# by #"nitrous acid"# to give #"sulfuric acid"#?
• How do you balance the following redox equation in acidic solution: #P_4 + HOCl -> H_3PO_4 + Cl^-#?
• Question #f0628
• Question #d0c67
• Question #6f8ee
• Question #3a2a3
• How to balance the following redox problems using both methods?
• How do you solve #I^- + ClO^- rarr I_3^- +Cl# using the redox reaction method in a base solution?
• How would we represent the oxidation of sucrose to give oxalic acid with nitric acid oxidant?
• How does #"iodic acid"#, #HIO_3#, react with iodide anion, #I^-#, to give elemental iodine?
• Question #75947
• How do you balance redox equations?
• What is the first step to balance a redox equation using the half-reaction method?
• How do we represent the oxidation of #Cr^(3+)# ion to #CrO_4^(2-)# by hydrogen peroxide, using the method of half-equations?
• Question #e3210
• Question #64b84
• What is the Balanced redox reaction for the following equation: I2 + Ca(ClO)2➡ Ca(IO3)2 +CaCl2 ?
• How do I balance this equation using the "half reaction" method: #CH_4+O_2+H_2O=CO+CO_2+H_2# ?
• Balance this reaction using ion electron method in shortest way possible . but must be clear .. #Fe^(2+)+MnO_4^(-)+H^(+) -> Fe^(3+)+Mn^(2+)+H_2O# ?
• Question #78b35
• Question #62a46
• Question #d49b8
• Question #c3e76
• How is #NO_2# oxidized by #Cr_2O_7^(2-)# to give nitrate ion?
• Question #06291
• Can you represent the reduction of tellurite ion, #TeO_3^(2-)#, to tellurium metal by the oxidation of iodide ion?
• How would you balance the following reactions using the oxidation number change method?
• Question #2bf15
• Question #6b532
• How to balance this redox reaction?
• How do we represent the oxidation of ethanol to acetic acid by potassium permanganate using the oxidation number method?
• Question #5e7c6
• Question #3ef9d
• Question #8470b
• What redox reaction occurs between #MnO_2# and #HCl#?
• How does aluminum metal react with nitrate ion under basic conditions to give ammonia, and aluminum ion?
• Question #be447
• Question #53cf1
• How do you write a balanced equation for this redox reaction using the smallest whole number coefficients?
• Question #e7fd5
• Question #065fa
• Question #412b9
• Balance each of the following half-reactions, assuming that they occur in basic solution?
• What is the balanced redox reaction between lead and ammonia?
• Balance this reaction? #"H"_ ((aq))^(+) + "MnO"_ (4(aq))^(2-) -> "MnO"_ ((aq))^(-) + "MnO"_ (2(s)) + "H"_ 2"O"_ ((l))#
• Balance the below in acidic solution (redox reaction)?
• Write a balanced redox equation for the following in acidic solution?
• Write a balanced oxidation reduction equation, in acidic solution, for the below reaction?