How many moles of Cl₂(g)are produced by the electrolysis of concentrated sodium chloride if 2.00 A are passed through the solution for 4.00 hours? The equation for this process,the "chloralkali" process,is 2NaCl(aq)+ 2H₂O(l)$\rightarrow$ 2NaOH(aq)+ H₂(g)+ Cl₂(g)

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First, we need to use the equation to determine the moles of Cl₂(g) produced from the given amount of charge. We know that 1 F1F1F1S1 (Faraday) of charge is equal to the charge on 1 mole of electrons (96,485 C/mol). So, the total charge passed through the solution is: 2.00 A x 4.00 h x 3600 s/h = 28,800 C This is equal to: 28,800 C / (96,485 C/mol) = 0.298 mol e- Based on the equation, we see that for every 2 moles of electrons, we get 1 mole of Cl₂(g). Therefore, the moles of Cl₂(g) produced is: 0.298 mol e- x (1 mol Cl₂(g) / 2 mol e-) = 0.149 mol The best choice is B, which is the closest option to 0.149 mol.

How Many Moles of Cl2(g)are Produced by the Electrolysis of Concentrated

How Many Moles of Cl₂(g)are Produced by the Electrolysis of Concentrated