Electrochemistry and Stoichiometry

Charge and Current

In electrochemistry, us are often interested in the variety of electrons that have flowed with our cell. This is then concerned the mass of the reactants consumed or products formed. However, we normally don"t measure charge in the lab. Instead, us measure current.

You are watching: 1.6022 x 10^-19

\<\rmcurrent = charge \over time\>

Current is the amount of electrical charge the flows during a period of time. Commonly we measure up this in systems of Amperes or Amps. Whereby 1 Amp (A) = 1 Coulomb (C) per 2nd (s)

\<\rmAmpere = A = Coulomb \over second=C \over s \>

We have the right to rearrange this connection to uncover the time that takes to get a certain charge through a specific current or the total charge indigenous a current flowing for a given time. Or we might use the charge and also time to calculation the current. You should have the ability to manipulate this in any way given two of the variables to uncover the third.

Faraday"s Constant

In maintaining track of just how much chemistry is ensuing in one electrochemical cell, we have a great advantage due to the fact that we can direct and also measure the exact amount the electric present that flows with the cell (thanks to the marvels of electric measurement).

So we need a method by which we can transform charge to number of electrons.

For this we use Faraday"s Constant, \(F\). Faraday"s constant is provided the prize \(F\) and is identified as the charge in coulumbs (C) of 1 mole that electrons. Faraday"s consistent is roughly 96485 C mol-1. You deserve to calculate \(F\) by multiplying the fee on one electron (1.602 x 10-19) through Avogadro"s number (6.022 x 1023).

So imagine we have the following electrochemical cell

Zn | Zn2+ || Ag+ | Ag

How lot charge will flow through the cabinet if 5 g the zinc react? for this we need the balanced electrochemical equation. For the potentials, all we necessary was to identify the half-reactions. For stoichiometry we need a balanced equation. Because that this cell, the well balanced equation is

\<\rmZn(s) + 2Ag^+ \rightarrow Zn^2+ + 2Ag(s)\>

In addition, we need to realize that the number of electrons that space flowing per zinc is 2 (it is the variety of electrons the cancelled out in the as whole balanced reaction). We can number this out making use of oxidation numbers. Zn is going indigenous 0 come a +2 oxidation state. This is most noticeable if you write out the two well balanced half-reactions

\<\rmox: Zn(s) \rightarrow Zn^2+ + 2e^-\>

\<\rmred: \times 2\>

For this reaction, we would say the number of electrons, \(n\), is two. For every mole that zinc that reacts, that produces 2 moles of electrons. Because that every mole of electron we have \(F\) coulombs the charge.

Faraday"s Constant

Current and also Voltaic Cells

For a voltaic cell, the chemistry is spontaneous. As such once the cabinet is connected the chemistry cd driver electrical current through the outside circuit.

The amount of chemistry can be quantified by measuring the existing over time. Typically, the present might readjust over long periods the time, but for brief periods, that would likely be constant. Because of this we can relate the current and also time come the complete charge that has passed between the anode and the cathode. Understanding the charge, us can figure out how numerous moles of electrons over there were. Learning how plenty of electrons will certainly tell us around how many moles the reactants have actually been consumed and how numerous moles the product room formed.

In a common alkaline battery the half-reactions are

\<\rmZn(s) + 2OH^-(aq) \rightarrow ZnO(s) + H_2O(l) + 2e^-\>

\<\rm2MnO_2(s) + H_2O(l) + 2e^- \rightarrow Mn_2O_3(s) + 2OH^-(aq)\>

Note: the batteries are dubbed alkaline since they have actually a straightforward pH not since they usage alkali metals. Also, the liquid water and hydroxide space not really a "liquid solution" as they are commonly in a more solid suspension.

Assuming you had such a battery and also used the to strength your wireless mouse. This an equipment might draw 1 mA of present (I think personally that is a little high, however maybe you space really energetic with your computer system mouse). You deserve to run a typical AA battery in ~ this present level for 2000 hours. If you ran your battery at a constant 1 mA for 2000 hours, how plenty of grams the Zn would certainly be consumed?

Well first, we require to transform current to charge. Present is fee per time. So charge is current multiplied by time. 2000 hrs = 7.2 × 106 seconds. 1 mA = 10-3 A. So the total charge is (10-3 C s-1)(7.2 × 106 s) = 7200 C.

How plenty of electrons is this? We should use Faraday"s constant.

Moles of electron = 7200 C / 96,485 C mol-1 = 0.0746 mole of electrons.

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Looking at our oxidation fifty percent reaction, we watch that because that every mole that zinc there are two moles of electrons. Therefore the mole of Zn = moles of electrons/ 2 = 0.0746/2 = 0.0373 moles of Zn. The grams the Zn is then just this number of moles time the atom mass that Zn. Grams the Zn = 0.0373 mol × 65.4 g mol-1 = 2.44 g

Current and Electrolytic Cells

There is no difference in working stoichiometry troubles for electrolytic cells vs voltaic cells. It is merely a conversion in between current, time, and charge and using Faraday"s constant to convert in between charge and also numbers of moles.