The kinetics of an electrochemical reaction involves analyzing the current-voltage polarization curves and the mass-specific activities of a fuel cell. The current-voltage polarization curve is a graphical representation that measures the kinetics of a reaction within the fuel cell with the equation P=IV (Power = Current x Voltage); the reaction's power will depend on the reaction's current and voltage. With the equilibrium potential being its maximum voltage, which occurs at 0 current, approximately 1.229 volts, the operating potential of the reaction will be lower due to inefficiencies caused by slow reaction kinetics. These inefficiencies can be characterized by the distance between the equilibrium potential and the actual current-voltage curve . Within the fuel cell, faster kinetics indicates a faster electrochemical reaction taking place at the electrode surfaces, specifically the oxygen reduction reaction. Fast kinetics will reduce the overpotential of the reaction, the additional voltage needed to drive a reaction at a certain rate. This reduction in overpotential minimizes energy wastage as heat, enhancing the efficiency of the conversion from hydrogen to electricity. Inversely, slow kinetics will increase the overpotential of the reaction, making the conversion between hydrogen and electricity less efficient .