Question

If you have 66.6 g nh3 how many grams of f2 are required for a complete reaction

Answer 1

To determine the amount of F2 required for a complete reaction with 66.6 g of NH3, we need to use the stoichiometry of the balanced chemical equation. Based on the mole ratio in the equation, approximately 148.6 grams of F2 are required.

Step-by-step explanation:

The question involves a chemical reaction between NH3 and F2. To determine the amount of F2 required for a complete reaction with 66.6 g of NH3, we need to use the stoichiometry of the balanced chemical equation. In the equation, NH3 and F2 have a one-to-one mole ratio, meaning that one mole of NH3 will react with one mole of F2. We can calculate the number of moles of NH3 by dividing the mass of NH3 by its molar mass. Then, we can use the mole ratio to find the number of moles of F2 needed. Finally, we can convert the moles of F2 back to grams by multiplying by its molar mass.

Example calculation:

1. Find the molar mass of NH3: 14.01 g/mol + 3(1.01 g/mol) = 17.03 g/mol
2. Calculate the number of moles of NH3: 66.6 g / 17.03 g/mol = 3.91 mol
3. Use the mole ratio to find the moles of F2: 3.91 mol NH3 * 1 mol F2 / 1 mol NH3 = 3.91 mol F2
4. Convert the moles of F2 back to grams: 3.91 mol F2 * 38.00 g/mol = 148.6 g F2

Therefore, approximately 148.6 grams of F2 are required for a complete reaction with 66.6 grams of NH3.

Answer 2

The correct answer is 186.1gF2

Step-by-step explanation:

Hello!

Let's solve this!

The reaction is:

2NH3 + 5F2 ---> N2F4 + 6HF

We have as data:

NH3 mass = 34g / mol

mass F2 = 95g / mol

mass NH3 = 66.6g

We don't use moles because we need mass in grams.

We calculate:

mass F2 = 66.6g * (95g / mol / 34g / mol) = 186.1gF2

The correct answer is 186.1gF2