# Problem: Calculate Eocell for the following balanced redox reaction.Br2(l) + 2I−(aq) → 2Br−(aq) + I2(s)Express your answer using two significant figures.

###### FREE Expert Solution

$\overline{){\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{cell}}}{\mathbf{=}}{\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{cathode}}}{\mathbf{-}}{\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{anode}}}}$

Recall:

Lose               Gain
Electron         Electrons
Oxidation       Reduction

cathode → reduction → oxidation number decreases

anode → oxidation → oxidation number increases

For ions: charge of the ion = oxidation number
For neutral atoms/compound: oxidation number = 0

Half-cell reactions:

• Br2(l) → 2Br(aq)
• charge changed from 0 to -1
• Br2 = 0, Br= -1
•  oxidation number decreased → gained electrons → reduced → cathode
• 2I(aq)   I2(s)
• charge changed from -1 to 0
• I= -1, I2 = 0
•  oxidation number increased → lost electrons → oxidized → anode
90% (94 ratings) ###### Problem Details

Calculate Eocell for the following balanced redox reaction.

Br2(l) + 2I(aq) → 2Br(aq) + I2(s)