Easy Practice — Set 2

Quick Recap — Electrochemical Cells

• Galvanic (voltaic) cell: oxidation at the anode (negative), reduction at the cathode (positive); electrons flow anode $\to$ cathode externally.
• $E^\circ_{cell}=E^\circ_{cathode}-E^\circ_{anode}$; a positive $E^\circ_{cell}$ means a spontaneous cell ($\Delta G=-nFE<0$).
• Standard hydrogen electrode $=0$ V (reference); $1\,F=96500$ C.
• Molar conductivity $\Lambda_m$ rises on dilution; Kohlrausch's law: $\Lambda^\circ_m=\lambda^\circ_++\lambda^\circ_-$.