A 2.0 molar aqueous solution of NaCl is prepared and 500 mL of this solution is electrolysed. This leads to the evolution of chlorine gas at one of the electrodes (atomic mass: Na = 23, Hg = 200, 1 faraday = 96500 coulomb). If the cathode is a Hg electrode, the maximum weight (in gram) of amalgam formed from this solution is a. 200 b. 225 c. 400 d. 446

Sure! Here are the step by step solutions: Given: $Na-Hg$ (amalgam) formed = 2 moles at cathode We can use the concept of Faraday's laws of electrolysis to solve this problem. Faraday's first law states that the amount of substance produced at an electrode is directly proportional to the amount of electricity passed through the electrolyte. Mathematically, it can be represented as: $Q=n\times F$ Where Q is the quantity of electricity passed, n is the number of moles of substance produced and F is the Faraday constant (96,485 C/mol). In this problem, we know that 2 moles of $Na-Hg$ amalgam is formed at the cathode. We can use this information to find the quantity of electricity passed. $n=2$ moles $F=96,485$ C/mol $Q=n\times F$$Q=2\times 96,485$$Q=192,970$ C Therefore, the quantity of electricity passed through the electrolyte is 192,970 C.