# 3SnCl4 + 4Al(C2H5)3  3Sn(C2H5)4 + 4AlCl3In one experiment, 0.270 L of SnCl4 (d = 2.226 g/mL) was treated with 0.521 L of triethylaluminum (Al(C2H5)3); d = 0.835 g/mL).What is the theoretical yield in this experiment (mass of tetraethylstannane, Sn(C2H5)4)? If 0.408 L of tetraethylstannane (d = 1.187 g/mL) were actually isolated in this experiment, what was the percent yield?

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3SnCl4 + 4Al(C2H5)3  3Sn(C2H5)4 + 4AlCl3

In one experiment, 0.270 L of SnCl4 (d = 2.226 g/mL) was treated with 0.521 L of triethylaluminum (Al(C2H5)3); d = 0.835 g/mL).
What is the theoretical yield in this experiment (mass of tetraethylstannane, Sn(C2H5)4)?

If 0.408 L of tetraethylstannane (d = 1.187 g/mL) were actually isolated in this experiment, what was the percent yield?

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Step 1

The mass and moles of SnCl4 and triethylaluminum is determined as follows,

Step 2

Observing the given balanced chemical equation clearly shows that 3 SnCl4 moles reacts with 4 Al(C2H5)3 and forms 3 moles of tetraethylstannane. About 1 mole of SnCl4  requires 4/3 moles of Al(C2H5)3 and  hence, 2.31 moles require...

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