Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride:

S (s) + 3F2 (g) SF6 (g)

What is the minimun number of moles of fluorine gas needed to completely react with 16 g sulfur?

a. 1
b. 1.5
c. 2
d. 3
e. 6

You didn't type in the arrow? How do we know the difference between the products and the reactants?

a. Convert 16 g S to moles. moles = grams/molar mass.
b. Using the coefficients in the balanced equation, convert moles S to moles fluorine.
Post your work if you get stuck.

To find the minimum number of moles of fluorine gas needed to completely react with 16 g of sulfur, we need to use the balanced chemical equation and convert grams of sulfur to moles.

The molar mass of sulfur is 32.06 g/mol, and we know that 16 g of sulfur is given. We can use this information to convert grams to moles:

16 g sulfur × (1 mol/32.06 g) = 0.4991 mol sulfur (rounded to four decimal places)

According to the balanced chemical equation, it shows that 1 mole of sulfur reacts with 3 moles of fluorine gas. Therefore, we can use this ratio to determine the minimum number of moles of fluorine gas needed:

0.4991 mol sulfur × (3 mol F2/1 mol S) = 1.4973 mol fluorine gas (rounded to four decimal places)

The minimum number of moles of fluorine gas needed is approximately 1.4973 mol. Since this value is closest to 1.5, the correct answer is option b. 1.5.