Electrolysis Calculator

Electrolysis calculations rely on Michael Faraday's foundational laws of electrochemistry, which connect electricity with chemical change. The core relationship states that the mass of a substance altered at an electrode is directly proportional to the total electrical charge passed through the substance. First, the total charge (Q) is determined by multiplying the electrical current (I) in amperes by the elapsed time (t) in seconds: Q = I * t. Next, the deposited or dissolved mass is calculated using the electrolysis constant, often represented by the electrochemical equivalent (Z), through the equation: mass = Z * Q. Combining these yields the comprehensive formula mass = Z * I * t.

Imagine you pass a steady electrical current of 5 amperes through an aqueous solution of silver salt for 30 minutes (1,800 seconds). Given that the electrochemical equivalent (constant) for silver is approximately 0.001118 grams per coulomb, we can find the total mass of silver deposited at the cathode. First, calculate the total charge passed: Q = 5 A * 1,800 s = 9,000 coulombs. Second, multiply this charge by the constant: mass = 0.001118 g/C * 9,000 C = 10.062 grams. Therefore, exactly 10.06 grams of pure silver will plate out onto the electrode.

Always ensure your time units are converted into seconds before performing calculations with amperes, as one coulomb equals one ampere-second. Pay close attention to the electrochemical equivalent value you select, as different oxidation states of the same element require distinct constants. Finally, account for current efficiency in real-world setups, because side reactions or heat losses often mean actual yields are slightly lower than theoretical maximums.