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Determine the overall reaction and its standard cell potential at 25 °C for the reaction involving the galvanic cell in which cadmium metal is oxidized to 1 M cadmium(II) ion and a half-cell consisting of an aluminum electrode in 1 M aluminum nitrate solution. Is the reaction spontaneous at standard conditions?
$\begin{aligned} 3 C d(s)+2 A l^{3+}(a q) & \rightarrow 3 C d^{2+}(a q)+2 A l(s) \\ E(c e l l) &=-1.259 V \end{aligned}$This reaction is not spontaneous.
Chemistry 102
Chapter 17
Electrochemistry
University of Central Florida
Rice University
Brown University
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mathematically standard cell potential is represented by the given equation easily equals, Eka told minus e an old let's re present this equation as number one. If the standard cell potential that is e cell is positive, then the reaction is a spontaneous. If negative, then the reaction will be known. Spontaneous. Consider the reaction in galvanic. Sit at a note. We have cadmium losing two electrons, whereas at cattle would we have aluminum gaining three elections. The overall reaction off the cell is represented by this chemical reaction substituting the values off E cathode Andi anode into equation one. We have value off standards. Cell potential equals negative 1.259 that is at 25 degree Celsius. The reaction is non spontaneous at given standard conditions.
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