How many molecules of BrF2 form when 384g Br2 react with excess F2?

equation: Br2 + 5F2 ---> 2BrF5

I really just need the guidelines to figure out the problem, i can figure out the rest from there. Please and thank you.

Answered below.

To find out how many molecules of BrF2 form when 384g Br2 react with excess F2, you can follow these steps:

1. Start by finding the number of moles of Br2 using its molar mass. The molar mass of Br2 is 159.808 g/mol. Divide the mass of Br2 (384g) by its molar mass to get the number of moles.

2. Once you have the number of moles of Br2, you can use the stoichiometry of the balanced equation to find the number of moles of BrF2. According to the balanced equation, 1 mole of Br2 reacts to form 2 moles of BrF2.

3. Finally, convert the number of moles of BrF2 into molecules by using Avogadro's number. Avogadro's number is 6.022 x 10^23 molecules/mol.

By following these steps, you should be able to determine how many molecules of BrF2 form.

To determine the number of molecules of BrF2 formed when 384g Br2 reacts with excess F2, we need to follow these steps:

1. Start with the given mass of Br2, which is 384g.
2. Use the molar mass of Br2 to convert the mass to moles. The molar mass of Br2 is 159.808 g/mol, so divide the mass by the molar mass:

384g Br2 * (1 mol Br2 / 159.808g Br2) = 2.4029 mol Br2

3. From the balanced chemical equation, we can see that the mole ratio between Br2 and BrF2 is 1:2. This means that for every 1 mole of Br2, we will have 2 moles of BrF2.
4. Use the mole ratio to determine the moles of BrF2 that will form:

2.4029 mol Br2 * (2 mol BrF2 / 1 mol Br2) = 4.8058 mol BrF2

5. To find the number of molecules of BrF2 formed, we need to convert moles to molecules. We can use Avogadro's number, which is 6.022 x 10^23 molecules/mol.

4.8058 mol BrF2 * (6.022 x 10^23 molecules BrF2 / 1 mol BrF2) = 2.894 x 10^24 molecules BrF2

Therefore, when 384g Br2 reacts with excess F2, approximately 2.894 x 10^24 molecules of BrF2 will be formed.