1) MnO2 + H+ + HNO2 ------> Mn+2 + H2O + NO3-
Oxidation half reaction : Addition of oxygen and removal of electrons :
HNO2 ---> NO3- + 2e-
N =+3 N = +5
Less number of oxygen atoms on lefts side so oxygen is added in the form of water
HNO2 + H2O ---> NO3- + 3 H+ + 2e- --------- 1
The substance that undergo oxidation is reducing agent - HNO2
Reduction half reaction : Removal of oxygen and addition of electrons :
MnO2 ----> Mn+2
+4 +2
Oxygen atoms are none on the right side so added on the left side in the form of water
MnO2 + 2e- + 4H+ ----> Mn+2 + 2H2O ------ 2
The substance that undergo reduction is oxidising agent - MnO2
Combine equations 1 and 2
HNO2 + H2O ---> NO3- + 3 H+ + 2e-
MnO2 + 2e- + 4H+ ----> Mn+2 + 2H2O
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HNO2 + MnO2 + H+ -------> Mn+2 + H2O + NO3-
2) HNO2 + Cr2O7-2 + H+ -------> Cr+2 + NO3- + H2O
Oxidation half reaction :
Addition of oxygen and removal of electrons :
HNO2 ---> NO3- + 2e-
N =+3 N = +5
Less number of oxygen atoms on lefts side so oxygen is added in the form of water
HNO2 + H2O ---> NO3- + 3 H+ + 2e- --------- 1
The substance that undergo oxidation is reducing agent - HNO2
Reduction half reaction : Removal of oxygen and addition of electrons :
Cr2O7-2 ----> Cr+2
Cr = +6 +2
There are no oxygen atoms on right hand side so added in the form of water
Cr2O7-2 ----> 2Cr+2 + 7H2O
Cr2O7-2 + 14H+ + 8e- ----> 2Cr+2 + 7H2O ------- 2
The substance that undergo reduction is oxidising agent - Cr2O7-2
Combine 1 and 2 :
HNO2 + H2O ---> NO3- + 3 H+ + 2e- x 4 ( to balance electrons)
4HNO2 + 4H2O ---> 4NO3- + 12 H+ + 8e-
Cr2O7-2 + 14H+ + 8e- ----> 2Cr+2 + 7H2O
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4HNO2 + Cr2O7-2 + 2H+ ----> 4NO3- + 2Cr+2 + 3H2O
118 HNO: Mn + H2O + NO MnO2 + H + Oxidation Half Reaction: Reduction Half...
i just need help with the problem that has been worked on. i dont think i did it right 3. MnO2 + H + HNO, Mn + -H Oxidation Half Reaction: Reduction Hall Reaction: Oxidizing agent: Reducing agent 4. PbO2 + Mn + S0- + H2O Dr H H MnO4 + → ___PbSO PbSO+ Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent 6 3 HNO2 + CrO2- +5H → 2Cr + 3 NO: + 4 H:0 Oxidation Half...
Oxidation H NO₂+ Fe + sor + H₂O Fes: Not pyrite) Oxidation Hall Reaction: Reduction Hall Reaction Oxidizing agent: Reducing agent 8. Mn + H2O + OH → MnO + H2O Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent MnO + NO + H2O → MnO2 + NO + OH Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent 10. Cl + OH CH + CO + H2O Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing...
i need help with these redox reactions H NO; + Re s or + H₂O Fes: NO, pyrite) Oxidation Hall Reaction: Reduction Half Reaction: Oxidizing agent Reducing agent Mn? + HO; + OH MnO + H2O Oxidation Half Reaction: Reduction Hall Reaction: Oxidizing agent: Reducing agent _MnO + NO + H2O → MnO: + NO + OH- Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent 0 Clz + OH - CH + CIO + H:0 Oxidation Half Reaction:...
Ner Reactions of Oridation Reduction Reactions: 1. CuSO. +_ 20,-- UUUUUUUUUUUUUU Observations Oxidation Half Reaction Reduction Half Reaction Net Reaction Oxidizing Agent Reducing Agent 2. HC+Zn -- Observations Oxidation Half Reaction Reduction Half Reaction Net Reaction Reducing Agent Oxidizing Agent NETTONIC AND REDUCTION OXIDATION REACTIONS pg. 187 FeSoin an acidic solution producing Manganese (11) and iron (1) ions * KMnO, Observations Oxidation Half Reaction Reduction Half Reaction LLL Net Reaction Oxidizing Agent Reducing Agent 4. KMnO, +K.CO in an acidic...
0.0257 in instead of In: 0.0592 logo MnO- + 1 . $-+ H2O → MO; + S8 + OH Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent 12. HS + NO:- + H → NO2 + S8 + H2O Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent 13. Zn + NO3- + H → Zn2+ + N2 + H2O Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent 14.__MnO4 + SO2 + H2O → SO42-...
i only need help with the curcled problems please 0 12 S 4 MnO,- + 12 s- + + 4 MnO2 + 3 Ss + 1LOH H2O H2O 4 MnO2 Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent 12. HS + NO:" + H N O2 + S8 + H20 Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent Not H 702 + + N₂ + H₂O Reduction Half Reaction: Oxidizing agent: Reducing agent 10. Bi(OH)3 +...
Classify each of the following half-equations as oxidation or reduction and balance. Also label the oxidizing agent and reducing agent for each reaction. a. (basic) (aq) Mn (aq) MnO2(s) (acidic)
Consider the chemical reaction below, KMnO4 + Na2SO3 + H2O → MnO2 + Na2SO4 + KOH Determine if each of the following statement is True or False. 1. The oxidation state of Mn in MnO2 is +2. 2. The oxidation state of S in Na2SO3 is the same as that in Na2SO4. 3. MnO4− gains electrons to form MnO23. 4. Na2SO3 is the oxidizing agent.
Balance the following ionic equations using the ion-electron method. Use H +1 and / or H2O, if necessary. Then identify the oxidation half-reaction and of reduction, the oxidizing agent and the reducing agent. 1. MnO4 - + H2C2O4 -2 → Mn + 2 + CO2 2. IO3 -1 + I-1 ⇌ I2 (ac)
Balance the redox reaction Reduction Half Reaction: Oxidizing agent: Reducing agent 9.MnO4 + _NO2 + _H2O → _MnO2 + __NO3- + _OH- Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent 10 Ci.