Calculate the value of E^∘ for each of the following reactions. Decide whether each is product-f

Calculate the value of E^∘ for each of the following...

Calculate the value of $E^{\circ}$ for each of the following reactions. Decide whether each is product-favored in the direction written. (a) $2 \mathrm{I}^{-}(\mathrm{aq})+\mathrm{Zn}^{2+}(\mathrm{aq}) \longrightarrow \mathrm{I}_{2}(\mathrm{s})+\mathrm{Zn}(\mathrm{s})$ (b) $\mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{Ni}(\mathrm{s}) \longrightarrow \mathrm{Zn}(\mathrm{s})+\mathrm{Ni}^{2+}(\mathrm{aq})$ (c) $2 \mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{Cu}^{2+}(\mathrm{aq}) \longrightarrow \mathrm{Cu}(\mathrm{s})+\mathrm{Cl}_{2}(\mathrm{g})$ (d) $\mathrm{Fe}^{2+}(\mathrm{aq})+\mathrm{Ag}^{+}(\mathrm{aq}) \longrightarrow \mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{Ag}(\mathrm{s})$

Calculate the value of $E^{\circ}$ for each of the following reactions. Decide whether each is product-favored in the direction written.
(a) $2 \mathrm{I}^{-}(\mathrm{aq})+\mathrm{Zn}^{2+}(\mathrm{aq}) \longrightarrow \mathrm{I}_{2}(\mathrm{s})+\mathrm{Zn}(\mathrm{s})$
(b) $\mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{Ni}(\mathrm{s}) \longrightarrow \mathrm{Zn}(\mathrm{s})+\mathrm{Ni}^{2+}(\mathrm{aq})$
(c) $2 \mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{Cu}^{2+}(\mathrm{aq}) \longrightarrow \mathrm{Cu}(\mathrm{s})+\mathrm{Cl}_{2}(\mathrm{g})$
(d) $\mathrm{Fe}^{2+}(\mathrm{aq})+\mathrm{Ag}^{+}(\mathrm{aq}) \longrightarrow \mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{Ag}(\mathrm{s})$

Key Concepts

Redox Reactions

Redox reactions are chemical processes that involve the transfer of electrons between species. These reactions consist of two simultaneous half-reactions – one undergoing oxidation (loss of electrons) and one undergoing reduction (gain of electrons) – and are central to the operation of batteries, corrosion, and various industrial applications.

Reaction Spontaneity

Reaction spontaneity in electrochemistry is determined by the sign of the standard cell potential. A positive E°cell indicates that a reaction is product-favored and will proceed spontaneously in the forward direction, whereas a negative value suggests non-spontaneity in that direction and that the reverse reaction would be favored.

Half-Reaction Method

The half-reaction method involves breaking down a redox reaction into its oxidation and reduction components. Each half-reaction is balanced separately for mass and charge before they are combined to form the overall balanced equation. This method is critical in determining the standard cell potential by matching and canceling electrons transferred in the process.

Standard Reduction Potentials

Standard reduction potentials are values assigned to half-reactions based on their tendency to gain electrons under standard conditions. These potentials, usually measured in volts, are tabulated to allow for the calculation of the overall cell potential when the appropriate half-reactions are combined in redox processes.

Standard Cell Potential

Standard cell potential, denoted as E°cell, is the measure of the driving force behind an electrochemical reaction under standard conditions. It is determined by the difference in the standard reduction potentials of the cathode and anode, and its sign indicates whether the reaction is spontaneous (positive E°cell) or non-spontaneous (negative E°cell) in the direction written.

Transcript

00:01 This problem is asking us to find the calculated electrochemical cell potential given some redox reactions.

00:11 Okay, so i compiled a list of reduction potentials from a table that i found online.

00:19 These values could possibly be different than the values that you use in your book, and that's okay.

00:26 The math and the way that you go about this problem is the exact same.

00:29 Just the numbers might be a little different.

00:31 So keep that in mind.

00:33 Okay, before we start, we need to go over one general equation, and that is cell potential is equal to reduction potential plus oxidation potential.

00:54 And that's really important, okay? another thing that we want to keep in mind is i found a table that only has reduction potentials.

01:03 If we want to find the oxidation potential, we just multiply the reduction potential by negative 1.

01:19 And with that, we can start with part a.

01:26 Oops, there we go.

01:27 Okay.

01:30 The first thing we need to do is we need to identify which atoms are being reduced and which atoms are being oxidized.

01:37 And we can do that by assigning oxidation states.

01:43 Iodine is going to have a negative 1 oxidation state because it has a minus 1.

01:47 One charge.

01:49 Zinc is going to have a plus two because it has a two plus charge...

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