# Problem: Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.)3 Cl2(g) + 2 Fe(s) → 6 Cl-(aq) + 2 Fe3+(aq) Cl2(g) + 2e- → 2 Cl-(aq)                      E° = +1.36 VFe3+(aq) + 3e- → Fe(s)                       E° = -0.04 VA) +4.16 VB) -1.40 VC) -1.32 VD) +1.32 VE) +1.40 V

###### FREE Expert Solution
88% (325 ratings)
###### FREE Expert Solution

cell    =    cathode   —   anode
(reduction)     (oxidation)

Usually:

• Larger E°cell = cathode
• Smaller E°cell = anode

BUT if an equation or a reaction is given:

88% (325 ratings)
###### Problem Details

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.)

3 Cl2(g) + 2 Fe(s) → 6 Cl-(aq) + 2 Fe3+(aq)

Cl2(g) + 2e- → 2 Cl-(aq)                      E° = +1.36 V
Fe3+(aq) + 3e- → Fe(s)                       E° = -0.04 V

A) +4.16 V

B) -1.40 V

C) -1.32 V

D) +1.32 V

E) +1.40 V

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

Our tutors have indicated that to solve this problem you will need to apply the Cell Potential concept. If you need more Cell Potential practice, you can also practice Cell Potential practice problems.

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Our tutors rated the difficulty ofUse the standard half-cell potentials listed below to calcul...as medium difficulty.

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Based on our data, we think this problem is relevant for Professor Bindell's class at UCF.