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Calculate the grams of Sr(s) produced when 2.54 Amperes are passed through the cell shown below for 9.81 hours. Sr^+2 (aq) + 2C1^-1 (aq) --> Sr(s) + Cl_2(g)

Answer :

Final answer:

The problem involves calculating grams of Sr(s) produced from a given current and time using principles of electrochemistry. Upon calculating the total charge passed through the cell, Faraday's law of electrolysis is used to determine the substance produced. The mass of strontium produced in this case is approximately 41.25 grams.

Explanation:

The process we need to calculate involves converting electrical energy into chemical change, this is a topic within electrochemistry. Given the current in Amperes and time in hours, the first step is to calculate total charge using the formula, Q=It, where I is current and t is time. Next, use Faraday's law of electrolysis, which states the amount of substance produced at the electrode during electrolysis is directly proportional to the quantity of electricity (charge) passed. In terms of mass, this relationship can be expressed as m = (Q/2F) * M, assuming it forms 2 moles of electrons as shown in the balanced chemical equation.

Plugging in the given numbers, the total charge Q = 2.54 A * 9.81 hr * 3600 s/hr = 91238.4 C. Using Faraday's constant F = 96485.34 C/mol and Molar mass of Sr = 87.62 g/mol, mass of Sr(s) produced = (91238.4 C / (2*96485.34 C/mol)) * 87.62 g/mol = 41.25 g.

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