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)

1.0 gTi; 1.0 gF2 Express your answer using two significant figures.

4.8 gTi; 3.2 gF2 Express your answer using two significant figures.

0.388 gTi; 0.341 gF2 Express your answer using three significant figures.

Answer 1

1) Given, the balanced chemical reaction,

Ti(s) + 2F₂(g) TiF₄(s)

Also given,

Mass of Ti = 1.0 g

Mass of F₂ = 1.0 g

Firstly, calculating the number of moles for the given masses of Ti and F₂,

= 1.0 g of Ti x ( 1 mol /47.867 g)

= 0.02089 mol of Ti

Similarly,

= 1.0 g of F₂ x ( 1 mol / 38.0 g)

= 0.02632 mol of F₂

Now, calculating the number of moles of F₂ required to react completely with the given moles of Ti,

= 0.02089 mol of Ti x (2 mol of F₂ / 1 mol of Ti)

= 0.04178 mol of F₂ is required to react completely with the given moles of Ti

Similarly,

= 0.02632 mol of F₂ x ( 1 mol of Ti / 2 mol of F₂)

= 0.01316 mol of Ti is required to react completely with the given number of moles of F₂.

Here, Moles of F₂ required to react completely with the given moles of Ti is more, hence, F₂ is the limiting reactant.

Now, using the moles of F₂ and the mole ratio from the balanced chemical reaction and calculating the number of moles of product forming,

= 0.02632 mol of F₂ x ( 1 mol of TiF₄ / 2 mol of F₂)

= 0.01316 mol of TiF₄

Converting the number of moles to grams,

= 0.01316 mol of TiF₄ x ( 123.861 g / 1mol)

= 1.6 g of TiF₄

2) Given, the balanced chemical reaction,

Ti(s) + 2F₂(g) TiF₄(s)

Also given,

Mass of Ti = 4.8 g

Mass of F₂ = 3.2 g

Firstly, calculating the number of moles for the given masses of Ti and F₂,

= 4.8 g of Ti x ( 1 mol /47.867 g)

= 0.1003 mol of Ti

Similarly,

= 3.2 g of F₂ x ( 1 mol / 38.0 g)

= 0.08421 mol of F₂

Now, calculating the number of moles of F₂ required to react completely with the given moles of Ti,

= 0.1003 mol of Ti x (2 mol of F₂ / 1 mol of Ti)

= 0.2006 mol of F₂ is required to react completely with the given moles of Ti

Similarly,

= 0.08421 mol of F₂ x ( 1 mol of Ti / 2 mol of F₂)

= 0.04210 mol of Ti is required to react completely with the given number of moles of F₂.

Here, Moles of F₂ required to react completely with the given moles of Ti is more, hence, F₂ is the limiting reactant.

Now, using the moles of F₂ and the mole ratio from the balanced chemical reaction and calculating the number of moles of product forming,

= 0.08421 mol of F₂ x ( 1 mol of TiF₄ / 2 mol of F₂)

= 0.04210 mol of TiF₄

Converting the number of moles to grams,

= 0.04210 mol of TiF₄ x ( 123.861 g / 1mol)

= 5.2 g of TiF₄

3) Given, the balanced chemical reaction,

Ti(s) + 2F₂(g) TiF₄(s)

Also given,

Mass of Ti = 0.388 g

Mass of F₂ = 0.341 g

Firstly, calculating the number of moles for the given masses of Ti and F₂,

= 0.388 g of Ti x ( 1 mol /47.867 g)

= 0.008106 mol of Ti

Similarly,

= 0.341 g of F₂ x ( 1 mol / 38.0 g)

= 0.008974 mol of F₂

Now, calculating the number of moles of F₂ required to react completely with the given moles of Ti,

= 0.008106 mol of Ti x (2 mol of F₂ / 1 mol of Ti)

= 0.01621 mol of F₂ is required to react completely with the given moles of Ti

Similarly,

= 0.008974 mol of F₂ x ( 1 mol of Ti / 2 mol of F₂)

= 0.004487 mol of Ti is required to react completely with the given number of moles of F₂.

Here, Moles of F₂ required to react completely with the given moles of Ti is more, hence, F₂ is the limiting reactant.

Now, using the moles of F₂ and the mole ratio from the balanced chemical reaction and calculating the number of moles of product forming,

= 0.008974 mol of F₂ x ( 1 mol of TiF₄ / 2 mol of F₂)

= 0.004487 mol of TiF₄

Converting the number of moles to grams,

= 0.004487 mol of TiF₄ x ( 123.861 g / 1mol)

= 0.56 g of TiF₄