Calculate the standard cell potential for the glavanic cell in which the follwoing reactino occurs:
2I^-(aq) + Br2(l) ---> I2(s) + 2Br^-(aq)
I^- ==> I2 E = ??
Br2 ==> Br E = ??
Add them together.
To calculate the standard cell potential for the given galvanic cell, you need to know the standard reduction potential values for the half-reactions involved in the reaction.
The half-reactions involved are:
1) I2(s) + 2e^- → 2I^-(aq) (reduction half-reaction)
2) Br2(l) + 2e^- → 2Br^-(aq) (oxidation half-reaction)
Step 1: Find the standard reduction potentials
Look up the standard reduction potentials for the half-reactions. These values are usually provided in reference tables or textbooks. Let's assume the values are:
E°red (I2/I^-) = +0.54 V
E°red (Br2/Br^-) = +1.07 V
Step 2: Identify the oxidation and reduction half-reactions
From the given reaction, we can see that I2(s) is being reduced to form I^- and Br2(l) is being oxidized to form Br^-. Therefore, the reduction half-reaction is 1) and the oxidation half-reaction is 2).
Step 3: Determine the overall cell potential
The standard cell potential (E°cell) can be calculated by taking the difference between the reduction potential of the cathode (reduction half-reaction) and the anode (oxidation half-reaction):
E°cell = E°red (cathode) - E°red (anode)
Since reduction is happening at the cathode, and oxidation is happening at the anode, we have:
E°cell = E°red (I2/I^-) - E°red (Br2/Br^-)
= (+0.54 V) - (+1.07 V)
= -0.53 V
Therefore, the standard cell potential for the galvanic cell is -0.53 V.