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.

You must mean BrF5.

Convert 384 g Br2 to moles.
Using the coefficients in the balanced equation convert moles Br2 to moles BrF5. Then 1 mol contains 6.02 x 10^23 molecules.

That's what I meant, thank you for you help DrBob222

Well, let me put my funny nose on for a second and guide you through this problem!

First things first, we need to convert the mass of Br2 into moles. And who doesn't love moles? They're like tiny furry creatures of chemistry!

So, we have 384g of Br2. Now, just to refresh your memory, the molar mass of Br2 is 159.808 grams/mol. So, we divide that 384g by the molar mass:

384g Br2 / 159.808 g/mol = 2.4018 mol Br2

And now that we have the number of moles of Br2, we can use the balanced equation to figure out the moles of BrF2 formed. According to the equation, for every 1 mole of Br2, we get 2 moles of BrF2.

So, if we have 2.4018 mol of Br2, we can multiply that by the ratio of BrF2 to Br2 to find the number of moles of BrF2 formed.

2.4018 mol Br2 * (2 mol BrF2 / 1 mol Br2) = 4.8036 mol BrF2

And there you have it! You will form approximately 4.8036 moles of BrF2 when 384g of Br2 reacts with excess F2. I hope that helps, and remember, chemistry jokes are always a good way to bond with your periodic table!

To find the number of molecules of BrF2 formed, we need to follow these steps:

1. Determine the molar mass of Br2 and BrF2.
2. Convert the mass of Br2 to moles.
3. Use the balanced chemical equation to determine the mole ratio between Br2 and BrF2.
4. Calculate the moles of BrF2 formed.
5. Convert moles of BrF2 to molecules using Avogadro's number.

Let's go through each step:

1. The molar mass of Br2 is 79.90 g/mol. The molar mass of BrF2 is 111.89 g/mol.

2. To convert the mass of Br2 to moles, divide the given mass (384 g) by the molar mass of Br2:

Moles of Br2 = 384 g / 79.90 g/mol

3. The balanced chemical equation shows that 1 mole of Br2 reacts to form 2 moles of BrF2. Therefore, the mole ratio between Br2 and BrF2 is 1:2.

4. Calculate the moles of BrF2 formed using the mole ratio:

Moles of BrF2 = Moles of Br2 * (2 moles of BrF2 / 1 mole of Br2)

5. Convert the moles of BrF2 to molecules using Avogadro's number. There are 6.022 x 10^23 molecules in 1 mole.

Number of molecules of BrF2 = Moles of BrF2 * Avogadro's number

By following these steps, you should be able to find the number of molecules of BrF2 formed when 384 g of Br2 react with excess F2.

To figure out the number of molecules of BrF2 formed when 384g Br2 reacts with an excess of F2, you need to follow these steps:

1. Convert the given mass of Br2 to moles. To do this, divide the given mass by the molar mass of Br2.

2. Use the balanced equation to establish the mole ratios between Br2 and BrF2. From the equation, you can see that 1 mole of Br2 reacts to form 2 moles of BrF2.

3. Calculate the number of moles of BrF2 formed. Multiply the number of moles of Br2 (calculated in step 1) by the mole ratio obtained from the balanced equation (2 moles of BrF2 / 1 mole of Br2).

4. Convert the moles of BrF2 to the number of molecules. The Avogadro's number is used to convert moles to the number of molecules. This constant is approximately 6.022 x 10^23 molecules per mole.

By following these steps, you can determine the number of molecules of BrF2 formed when 384g Br2 reacts with an excess of F2.