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Calculate the grams of [tex]Sr(s)[/tex] produced when 4.79 Amperes are passed through the cell for 5.79 hours.

\[ Sr^{2+}(aq) + 2Cl^−(aq) \rightarrow Sr(s) + Cl_2(g) \]

Answer :

To calculate the grams of Sr(s) produced, use the formula Q = nF, where Q is the charge passed through the cell, n is the number of moles of electrons transferred, and F is Faraday's constant. Using the given charge of 27.7641 C, you can calculate the moles of electrons and then use the balanced equation to find the moles of Sr(s) .

To calculate the grams of Sr(s) produced, we need to use the formula:

Q = nF

Where Q is the charge passed through the cell, n is the number of moles of electrons transferred, and F is Faraday's constant (96485 C/mol e-).

Given that the charge passed through the cell is 4.79 Amperes * 5.79 hours = 27.7641 C, we can calculate the moles of electrons:

n = Q / F = 27.7641 C / 96485 C/mol e- = 0.000287 mol e-

Since the balanced equation tells us that 2 mol e- are required to produce 1 mol of Sr(s), we can calculate the moles of Sr(s) produced:

moles of Sr(s) = 0.000287 mol e- / 2 mol e-/1 mol Sr(s) = 0.0001435 mol Sr(s)

Finally, we can calculate the grams of Sr(s) produced using the molar mass of Sr:

mass of Sr(s) = 0.0001435 mol Sr(s) * 87.62 g/mol = 0.01256 g Sr(s)

Learn more about gram calculation here:

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