In the electrolysis of an acid solution, oxygen can be produced by the following half-reaction: 2H2O(l) → O2(g) + 4H+(aq) + 4e– How much time (min) is required to collect 12.1 L of oxygen, using a current of 5.49 A, if the gas is collected over water at 22.0°C and the total pressure is 95.5 kPa? Assume that the water is already saturated with oxygen so no more dissolves. Assume Ptotal(gas)  =  P(O2,g)  +  P(H2O,g) and that the correction for column height is negligible. The vapor pressure of water at 22.0°C is 2.643 kPa, F = 96485 C/mol e-. and R = 8.314 kPa·L·mol-1·K-1 Enter your final answer for the time required in units of minutes. Include only the numerical answer

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.