<p>A student places a copper electrode in a 1 M solution of CuSO4 and in another beaker places a silver electrode in a 1 M solution of AgNO3. A salt bridge composed of Na2SO4 connects the two beakers. The voltage measured across the electrodes is found to be +0.42 volt.</p>
<p>How do you write balanced overall cell equation for this problem and the standard cell notation??</p>
<p>One side contains 1 M Cu+2 / the Other side contains 1 M Ag+</p>
<p>Since Ag doesn’t go to Ag+2, you assume Ag+ will go to plain old Ag instead. That’s a reduction in charge from +1 to 0. Because redox reactions always have oxidation and reduction go hand in hand, you know the other reaction has to be an oxidation reaction involving the copper, because the Ag+ is reduced. </p>
<p>So Cu+2 will be oxidized (get more positive) to the next usual state, which is Cu+3. </p>
<p>To write the balanced redox reaction, you must write down the half reactions that occur in each of the two cells. </p>
<p>electron + Ag+ –> Ag
Cu+2 –> Cu+3 + electron</p>
<p>You must now check that 1. on one equation the electron(s) are on the left side, and on the other reaction the electron is on the other side, and 2. the same number of electrons are reacting in both reactions. if not, then you need to multiply one of the reactions with a constant. these two reactions are fine. </p>
<p>Add them together to get </p>
<p>electron + Ag+ + Cu+2 –> Ag + Cu+3 + electron</p>
<p>The electrons cancel out and you get </p>
<p>Ag+ + Cu+2 –> Ag + Cu+3</p>
<p>That’s the balanced redox reaction.</p>
<p>so what’s the the standard cell notation?? is balanced “redox” equation same as balanced “overall cell equation”??</p>