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

Answer :

joseaaronlara

Answer:

The answer to your question is 8.2 g of TiF₄

Explanation:

Data

Theoretical yield = ?

mass of Ti = 5 g

mass of F₂ = 5 g

Balanced chemical reaction

                  Ti(s) +  2F₂ (g)   ⇒   TiF₄(g)

Process

1.- Calculate the Molar mass of reactants and products

Ti = 48 g

2F₂ = 2( 19 x 2) = 76 g

TiF₄ = 48 + 76 = 124 g

2.- Calculate the limiting reactant

theoretical proportion Ti/F₂  = 48/76 = 0.63

experimental proportion Ti/F₂ = 5/5 = 1

Conclusion The limiting reactant is F₂ because the experimental proportion was lower than the theoretical proportion.

3.- Calculate the theoretical yield using the mass of F₂

                   76 g of F₂ --------------- 124 g of TiF₄

                     5 g of F₂ ---------------  x

                      x = (5 x 124) / 76

                      x = 8.15 g of TiF₄

The theoretical yield of the product (in grams) is 8.1 g

The given chemical equation of reaction is

Ti(s) + 2F₂(g) → TiF₄(s)

This means

1 mole of Ti reacts with 2 moles of F₂ to produce 1 mole of TiF₄

Now, we will determine the number of moles of each reactant present.

  • For Titanium (Ti)

Mass = 5.0 g

Atomic mass = 47.867 g/mol

From the formula

[tex]Number\ of\ moles = \frac{Mass}{Atomic\ mass}[/tex]

∴ Number of moles of Ti present = [tex]\frac{5.00}{47.867}[/tex]

Number of moles of Ti present = 0.104456 mol

  • For Fluorine (F₂)

Mass = 5.0 g

Molar mass of fluorine = 37.9968 g/mol

∴ Number of moles of F₂ present = [tex]\frac{5.0}{37.9968}[/tex]

Number of moles of F₂ present = 0.13159 mol

Now,

Since 1 mole of Ti reacts with 2 moles of F₂

Then,

[tex]\frac{0.13159}{2}[/tex] mole of Ti will react with the 0.13159 mole of F₂

[tex]\frac{0.13159}{2} = 0.065795[/tex]

∴ Only 0.065795 mole of Ti reacted

From the balanced chemical equation,

1 mole of Ti reacts with 2 moles of F₂ to produce 1 mole of TiF₄

Then,

0.065795 mole of Ti will react with the 0.13159 mole of F₂ to produce 0.065795 mole of TiF₄

∴ The number of mole TiF₄ produced is 0.065795 mole

Now, for the mass of the product, TiF₄

From the formula

Mass = Number of moles × Molar mass

Molar mass of TiF₄ = 123.861 g/mol

∴ Mass of TiF₄ produced = 0.065795 × 123.861

Mass of TiF₄ produced = 8.14943 g

Mass of TiF₄ produced ≅ 8.1 g

Hence, the theoretical yield of the product (in grams) is 8.1 g

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