Electrolytic cell

<p>An electrolytic cell is an <a href="/facts/Electrochemical_cell/o7oEnYVl">electrochemical cell</a> that uses an external source of <a href="/facts/Electrical_energy/V0pJUrDY">electrical energy</a> to drive a non-spontaneous <a href="/facts/Chemical_reaction/GpqWlKrz">chemical reaction</a>, a process known as <a href="/facts/Electrolysis/pU75nCDI">electrolysis</a>.: 64, 89 : GL7  In the cell, a <a href="/facts/Voltage/EN2po6N2">voltage</a> is applied between the two <a href="/facts/Electrode/251PaKX8">electrodes</a>—an <a href="/facts/Anode/TjYt95zG">anode</a> (positively charged) and a <a href="/facts/Cathode/tqdlGayU">cathode</a> (negatively charged)—immersed in an <a href="/facts/Electrolyte/4YE8bIVa">electrolyte</a> solution.: 89  This contrasts with a <a href="/facts/Galvanic_cell/a4V7CQC8">galvanic cell</a>, which produces electrical energy from a <a href="/facts/Spontaneous_process/xyGhdUG0">spontaneous</a> chemical reaction and forms the basis of <a href="/facts/Electric_battery/bqEpm4ue">batteries</a>.: 64  The net reaction in an electrolytic cell is a non-spontaneous (<a href="/facts/Gibbs_free_energy/bvenDuzh">Gibbs free energy</a> is positive), whereas in a galvanic cell, it is spontaneous (Gibbs free energy is negative).
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Electrolytic cell open-in-new

Electrolytic cell