Balance the following equations under the solution conditions of
acid or base as indicated:
a) MnO4- (aq) + Br- (aq) --> Br3- (aq) + MnO2 (g) acid
b) Br2 (l) + IO3- (aq) --> IO4- (aq) + Br- (aq) basic
Balance the following equations under the solution conditions of acid or base as indicated:
a) MnO4- (aq) + Br- (aq) --> Br3- (aq) + MnO2 (g) acid
The balance reaction is as follows:
Br- (aq) + 2 MnO4- (aq) +2H+ ---- > BrO3- + 2MnO2 (g) +H2O
b) Br2 (l) + IO3- (aq) --> IO4- (aq) + Br- (aq) basic
The balance reaction is as follows:
H2O + + IO3- (aq)+ Br2 (l) --- > IO4- (aq) + 2 Br- (aq) +2H+
Balance the following equations under the solution conditions of acid or base as indicated: a) MnO4-...
Balance Redox Equations (Basic Solution) with steps. 1. Mn^2+ (aq) + Br2(l) = MnO2 (s) + Br^- (aq) 2. NO2^- (aq) + MnO4^- (aq) = NO3^- (aq) + MnO2 (s) 3. N2H4 (g) + ClO3^- (aq) = NO(g) + Cl^- (aq)
Balance the redox equations: a. CO2+ Mn2+→H2C2O4+ MnO4- (in basic conditions) b. Br- + MnO4 ----> MnO2+ BrO3- (in acidic conditions) Please show all steps and explain
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)
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)
2. Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): MnO (s) + PbO2 (s) → MnO,- + Pb2+ (b) (acid solution): MnO4 + Mn2+ → MnO2 (s) (c) (basic solution): Al (8) + OH → Al(OH) - + H2(g)
Complete and balance the following redox reaction in basic solution MnO4-(aq) + Br-(aq) → MnO2(s) + BrO3-(aq) Attempts remaining: 3 Complete and balance the following redox reaction in basic solution 103-(aq) + Re(s) → Re04 (aq) + 10-(aq) Attempts remaining: 3
Balance the following redox reactions: a) CN− + MnO4− → CNO− + MnO2 (basic solution) b) O2 + As → HAsO2 + H2O (acidic solution) c) Br− + MnO4− → MnO2 + BrO3− (basic solution) d) NO2 → NO3− + NO (acidic solution) e) ClO4− + Cl− → ClO− + Cl2 (acidic solution) f) AlH4− + H2CO → Al3+ + CH3OH (basic solution)
Question 1 (1 point) Balance the following reaction which occurs under acidic conditions. What is the balanced reaction? Ag (s) + NO3(aq) -- Ag+ (aq) + NO (g) O Ag (s) + 4 NO3- (aq) +8H* -- Ag+ (aq) + 4 NO(g) + 4 H20 (1) 3 Ag (s) + NO3- (aq) + 4H+ (aq)- 3 Ag+ (aq) + NO (g) + 2 H20 O Ag (s) + NO3(aq) + 4H+ -- Ag+ (aq) + NO (g) + 2 H20...
What is the expected standard cell potential for the following unbalanced reaction under basic conditions? MnO4-(aq) + Fe+2(aq) ⟶ Fe+3 (aq) + MnO2(s) Given: Fe3+ + e− ⟶ Fe2+ E1/2= 0.771 MnO4−+ 2 H2O + 3e− ⟶ MnO2 + 4OH− E1/2 = 0.558 A. -0.213 V B. +0.213 V C. -1.329 V D. +1.329 V E. None of the above
Problem 2. Complete and balance the following equations for the reactions occurring in basic solution: a. MnO4-(aq)+C2O42-(aq)→MnO2(s)+CO2(g) b. NO2-(aq) + Al(s) → NH3(g) + Al(OH)4-(aq) Answer: a. 4H2O + 2MnO4- + 3C2O42- → 2MnO2 + 8OH- + 6CO2 b. 5H2O + NO2- + OH- + 2Al → NH3+ 2Al(OH)4-