For the reaction shown, compute the theoretical yield of the product (in grams)

Question

For the reaction shown, compute the theoretical yield of the product (in grams) for each of the following initial amounts of reactants. Ti(s) + 2F2(g) ----> TiF4(s) 5.0g Ti, 5.0g F2 Express your answer using two significant figures.

Explanation / Answer

Ti(s) + 2F2(g) ----> TiF4(s) molar mass: Ti = 48 g/mol F2 = 38 g/mol TiF4 = 124 g/mol moles of Ti = 5.0/48 = 0.10 mol moles of F2 = 5.0/38 = 0.13 mol since the molar ratio of Ti : F2 = 1 : 2 Ti is in excess and F2 is the limiting reagent. Then we use the amount of F2 to calculate the yield. moles of TiF4 = moles of F2/2 = 0.13/2 = 0.065 mol theoretical yield = moles of TiF4 x molarity of TiF4 = 0.065 x 124 = 8.1 g

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