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Problem: Consider the following reaction and select the false statement below.NaI + 3HOCl → NaIO3 + 3HClA. HOCl is the oxidizing agentB. Cl is reducedC. NaI is the reducing agentD. If ΔG° for the reaction is < 0, then NaI is a stronger reducing agent than HClE. If ΔG° for the reaction is < 0, then NaIO3 is a stronger oxidizing agent than HOCl

FREE Expert Solution

To identify the false statement:


Recall the mnemonic for redox reactions:

Loss Electrons Oxidation Reducing Agent

Gain Electrons Reduction Oxidizing Agent


This means the element that gains electrons/reduced is the oxidizing agent while the element that loses electrons/oxidized is the reducing agent


Recall that if:

• ΔG < 0 or ΔG = (–); the reaction is spontaneous

• ΔG = 0; the reaction is at equilibrium

• ΔG > 0 or ΔG = (+); the reaction is non-spontaneous


Step 1: Oxidation Numbers

  • NaI 
    • O.S. of Na → Group 1A: O.S. = +1 
    • O.S. of I (not bonded to O) → Group 7A: O.S. = -1 
  • HOCl → halogen, Cl is bonded to O
    • O.S. of H (with nonmetals)→ Group 1A: O.S. = +1 
    • O.S. of O (not a peroxide) → Group 6A: O.S. = -2 
  • sum of O.S. = 0 → neutral compound
    • O.S. of Cl, x 
    • (+1) + (-2) + x = 0 
    • x = 2 - 1  
    • O.S. of Cl = +1
  • NaIO3 → halogen, I is bonded to O
    sum of O.S. = 0 → neutral compound
    • O.S. of I, x 
    • (+1) + x + 3(-2) = 0 
    • x = 6 - 1  = +5
    • O.S. of I = +5
  • HCl
    • O.S. of H  = +1 
    • O.S. of Cl (not bonded to O)  = -1 
  • Changes in O.S.
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Problem Details

Consider the following reaction and select the false statement below.

NaI + 3HOCl → NaIO3 + 3HCl

A. HOCl is the oxidizing agent

B. Cl is reduced

C. NaI is the reducing agent

D. If ΔG° for the reaction is < 0, then NaI is a stronger reducing agent than HCl

E. If ΔG° for the reaction is < 0, then NaIO3 is a stronger oxidizing agent than HOCl

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What scientific concept do you need to know in order to solve this problem?

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