# 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 &lt; 0, then NaI is a stronger reducing agent than HClE. If ΔG° for the reaction is &lt; 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.
93% (460 ratings) ###### 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