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 above.
To figure out the number of molecules of BrF2 formed when 384g of Br2 reacts with excess F2, you need to follow these steps:
Step 1: Determine the number of moles of Br2.
To do this, you need to use the molar mass of Br2, which is 159.808 g/mol. Divide the given mass (384g) by the molar mass to find the number of moles of Br2.
Number of moles of Br2 = mass of Br2 / molar mass of Br2
Step 2: Use the balanced chemical equation to find the mole ratio between Br2 and BrF2.
From the balanced equation, you can see that the mole ratio between Br2 and BrF2 is 1:2.
This means that for every 1 mole of Br2, 2 moles of BrF2 are produced.
Step 3: Convert the number of moles of Br2 to moles of BrF2.
Multiply the number of moles of Br2 by the mole ratio from Step 2 to find the number of moles of BrF2 produced.
Number of moles of BrF2 = number of moles of Br2 x mole ratio of Br2 to BrF2
Step 4: Convert the number of moles of BrF2 to the number of molecules.
To convert moles to molecules, you need to use Avogadro's number, which is 6.022 x 10^23 molecules/mol. Multiply the number of moles of BrF2 by Avogadro's number to calculate the number of molecules of BrF2.
Number of molecules of BrF2 = number of moles of BrF2 x Avogadro's number
Now, you can use these guidelines to calculate the number of molecules of BrF2 formed when 384g of Br2 reacts with excess F2.