Complete and balance the following redox reactions in acidic medium, be sure to label the oxidizing and reducing agents in each.
S(s) + HNO3(aq) → H2SO3(aq) + N2O(g)
BrO3 - (aq) + N2H4(g) → Br- (aq) + N2(g)
Complete and balance the following redox reactions in basic medium, be sure to label the oxidizing and reducing agents in each.
NO2 - (aq) + Al(s) → NH4 + (aq) + AlO2 - (aq)
H2O2(aq) + ClO2(aq) → ClO2 - (aq) + O2(g)
BALANCED EQUATION:
The half-reactions are;
Half oxidation reaction | Half reduction reaction |
As the reaction is taking place in acidic medium,proton and water molecules can be added in either side of the reaction followed by the charge balancing by electron addition.
after balancing the half equations,we get-
.........eq.1
........eq.2
after balancing these two equation, we get,
here,Oxidising agent is HNO3(aq) and Reducing agent is S(s)
Half oxidation reaction | Half reduction reaction |
As the reaction is taking place in acidic medium,proton and water molecules can be added in either side of the reaction followed by the charge balancing by electron addition.
after balancing the half equations,we get-
.......eq.1
......eq.2
after balancing these two equation, we get,
Here Oxidising agent is BrO3-(aq) and reducing agent is N2H4(g)
Half oxidation reaction | Half reduction reaction |
As the reaction is taking place in basic medium,hydroxide ion and water molecules can be added in either side of the reaction followed by the charge balancing by electron addition.
after balancing the half equations,we get-
.......eq.1
.....eq.2
after balancing these two equation, we get,
here,the oxidising agent is NO2-(aq) and the Reducing agent is Al(s)
Half oxidation reaction | Half reduction reaction |
As the reaction is taking place in basic medium,hydroxide ion and water molecules can be added in either side of the reaction followed by the charge balancing by electron addition.
after balancing the half equations,we get-
....eq.1
........eq.2
after balancing these two equation, we get,
here the Oxidising agent is ClO2 and the reducing agent is H2O2
Complete and balance the following redox reactions in acidic medium, be sure to label the oxidizing...
Redox Reactions: Balance the reaction and determine which is the oxidizing and reducing agent in each case. 2. Cr* + Sn" Cr: Sn + 3. NaBr + Cl2 → NaCl + Br2 MnO,(s) (basic O2 (g) + 5. MnO (aq) H2O2 (aq) medium) 6. Cr2O72- → Cr+ (aq) SO2 SO2 (aq) (acidic)
BALANCE and FIND the half-reactions for this Redox Reaction, then indicate which substances are Oxidizing Agents, and Reducing Agents. Fe^3+(aq) + NH2OH2+(aq) = Fe^2+(aq) + N2O(g)
balance the following half-reactions (all of which take place in acidic solution) a. HClO(aq) ---> CL^-(AQ) b. NO(AQ)--->N2O(G) c. N2O(AQ)--->N2(G) d. CLO3^-(AQ--->HCLO2(AQ) e. O2(G)--->H2O(L) f. SO4^2^-(AQ)--->H2SO3(AQ) g. H2O2(AQ)--->H2O(L) h. NO2^-(AQ)--->NO3^-(AQ)
BALANCE the redox equation in a BASIC solution and FIND the oxidizing and reducing agents: CrI3(s) + H2O2(aq) = CrO4^2-(aq) + IO4-(aq) The equation is in an acidic solition
5) Balance the following redox reactions. For each one, identify the reducin and the oxidizing agent. (acidic solution) a) Cr2O72- + NO2 = Cr3+ + NO3- (basic solution) b) H O2 + Cio2 = 02 + ClO2- (acidic solution) c) Mnox + VÕ2+ = Mn2+ + V(OH)4* d) AIS) + Noz = NH4+ + A102 (basic solution) e) 103- + 1 = 12 (acidic solution) f) SCN-+ Br03- = Br + SO42- + HCN (acidic solution)
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 each of the following redox reactions in basic solution. 18.34 Balance each of the following redox reactions in basic solution. (a) CIO-(aq) + CrO(aq) → C1- (aq) + Cro (aq) (b) Br2(aq) + Br (aq) + BrO3(aq) (c) H2O2(aq) + N H(aq) → N2(g) + H2O(O)
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 redox reaction in acidic solution. BrO3 + N2H4 - Br" + N2
Balance the following redox reactions. For each one, identify the reducing agent and the oxidizing agent. SCN– + (BrO3)– --> Br– + (SO4)2– + HCN