Question

What mass of F2 is needed to yield 0.178 moles of ferric fluoride FeF3 given the reaction 2 Fe + 3 F_2 rightarrow 2 FeF_3?

A. 10.67 g

B. 20.0 g

C. 30.0 g

D. 40.0 g

Answer 1

To find the mass of F2 needed to yield 0.178 moles of FeF3, we need to use the stoichiometry of the balanced chemical equation and calculate the moles and then the mass of F2.

Step-by-step explanation:

To find the mass of F2 needed to yield 0.178 moles of FeF3, we need to use the stoichiometry of the balanced chemical equation. The equation shows that 2 moles of Fe react with 3 moles of F2 to produce 2 moles of FeF3. Therefore, the mole ratio of F2 to FeF3 is 3:2. Given that there are 0.178 moles of FeF3, we can calculate the moles of F2 using the mole ratio.

(moles of F2) = (moles of FeF3) × (2/3)

(moles of F2) = 0.178 × (2/3) = 0.11867 moles

Now, to find the mass of F2, we can use its molar mass which is 38.00 g/mol.

(mass of F2) = (moles of F2) × (molar mass of F2)

(mass of F2) = 0.11867 × 38.00 = 4.50746 g

Therefore, the mass of F2 needed to yield 0.178 moles of FeF3 is approximately 4.51 g.