Redox and balancing equation

Which species could be reduced to form NO₂?

• N₂O

    

• NO₃^-

      

• HNO₂

     

• NO

What happens to bromine when bromate ions, BrO₃^- , are converted to bromine molecules, Br₂?

•  It undergoes reduction and its oxidation state changes from -1 to  0.

   

•  It undergoes oxidation and its oxidation state changes from - 1 to 0.

• It undergoes reduction and its oxidation state changes from +5 to O.

• It undergoes oxidation and its oxidation state changes fron1 +5 to O

What is the reducing agent in the reaction below?

2MnO₄ (aq) + Br ^- (aq) + H₂O(l) → 2MnO₂(s) +BrO₃^-+ 2OH^-(aq)

• Br ^–

   

•  BrO₃^-  

• MnO₄^-

    

• MnO₂

Which compound contains chlorine with the highest oxidation number?

•     NaCl

• HOCl

   

• Cl₂O₇

    

• ClF

Which of the following is not a redox reaction?

•    Zn(NO₃)₂(aq) + Mg(s) → Mg(NO₃)₂(aq) + Zn(s)

• U(s) + 6ClF(l)  →  UF₆(l) + 3Cl₂(g)

• 2NO₂(g)  →  N₂O₄(g)

• 2SO₂(g)  +  O₂(g) →  2SO₃(g)

Balance the following redox equations for reactions that occur in neutral solution:

Zn + Ag+ → Zn²⁺ + Ag

•   Zn + 2Ag⁺ →  Zn²⁺ + 2Ag

    

• Zn + Ag⁺ →  Zn²⁺ + Ag

•   Zn + 2Ag⁺ → Zn²⁺ + Ag

• Zn+ Ag⁺ → 2 Zn²⁺ + 2Ag

Balance the following redox equations for reactions that occur in neutral solution:

Fe³⁺ + I⁻ → Fe²⁺ + I_2. :

• Fe³⁺ + 2I⁻ →  Fe²⁺ + 2I₂

• Fe³⁺ +  I⁻ →  Fe²⁺ + I₂

• 2Fe³⁺ + I⁻ →  2Fe²⁺ + I₂

• 2Fe³⁺ + 2I⁻ →  2Fe²⁺ + I₂

Balance the following half-equations for reactions that occur in acidic solution:

BrO₃⁻ + I⁻ → Br₂ + I₂

• 2BrO₃⁻ + 10I⁻ + 6H⁺ → Br₂ + 5I₂ + 3H₂O

• 2BrO₃⁻ + 10I⁻ + 12H⁺ → Br₂ + 5I₂ + 6H₂O

• BrO₃⁻ + 10I⁻ + 14H⁺ → Br₂ + 5I₂ + 7H₂O

• BrO₃⁻ + 5I⁻ + 12H⁺ → Br₂ + 3I₂ + 6H₂O

Balance the following half-equations for reactions that occur in acidic solution :

Zn + VO²⁺ + H⁺ → V³⁺ + H₂O + Zn²⁺

• Zn + 2VO²⁺ + 4H⁺ → Zn²⁺ + 2V³⁺ + 2H₂O

     

• Zn + VO²⁺ + 4H⁺ → Zn²⁺ + V³⁺ + 2H₂O

• Zn + 2VO²⁺ + 2H⁺ → Zn²⁺ + 2V³⁺ + H₂O

• 2Zn + 2VO²⁺ + 4H⁺ → Zn²⁺ + 2V³⁺ + 2H₂O