Some electrode potential data are shown:
Cr3+(aq)+3e−→Cr(s)E⊖=−0.74 V \text{Cr}^{3+}(\text{aq}) + 3\text{e}^- \rightarrow \text{Cr}(\text{s}) \quad E^\ominus = -0.74\text{ V} Cr3+(aq)+3e−→Cr(s)E⊖=−0.74 V Cu2+(aq)+2e−→Cu(s)E⊖=+0.34 V \text{Cu}^{2+}(\text{aq}) + 2\text{e}^- \rightarrow \text{Cu}(\text{s}) \quad E^\ominus = +0.34\text{ V} Cu2+(aq)+2e−→Cu(s)E⊖=+0.34 VAn electrochemical cell is set up as represented below:
Cr(s)∣Cr3+(aq)∥Cu2+(aq)∣Cu(s) \text{Cr}(\text{s}) \mid \text{Cr}^{3+}(\text{aq}) \parallel \text{Cu}^{2+}(\text{aq}) \mid \text{Cu}(\text{s}) Cr(s)∣Cr3+(aq)∥Cu2+(aq)∣Cu(s)Which is a correct statement about this cell?
The standard EMF of the cell is +0.40 V+0.40\text{ V}+0.40 V.
Electrons flow through the salt bridge from the chromium electrode to the copper electrode.
Anions from the salt bridge migrate into the chromium half-cell to maintain electrical neutrality.
The concentration of chromium(III) ions decreases as the cell discharges.
