Question

Fluorine reacts with sulfur to produce sulfur hexafluoride (SF6).

S + 3F2 → SF6
Relative formula masses, Mr: F2 = 38 SF6 = 146
Calculate the mass of sulfur hexafluoride produced when 0.950 g of fluorine is reacted with an excess of sulfur.

Answer 1

To calculate the mass of sulfur hexafluoride produced, we need to determine the number of moles of fluorine reacted and then use the stoichiometry of the reaction to find the moles of sulfur hexafluoride produced. Finally, we can calculate the mass using the molar mass of sulfur hexafluoride.

Step-by-step explanation:

First, we need to calculate the molar mass of fluorine (F2) and sulfur hexafluoride (SF6). The molar mass of F2 is 2 x 19 = 38 g/mol.

The molar mass of SF6 is 1 x 32 + 6 x 19 = 146 g/mol.

Next, we need to determine the number of moles of fluorine in 0.950 g. We can use the formula: moles = mass / molar mass. So, moles of F2 = 0.950 g / 38 g/mol = 0.025 moles.

Since the reaction between fluorine and sulfur has a 1:1 stoichiometry, we know that 0.025 moles of sulfur hexafluoride will be produced. Finally, we can calculate the mass of sulfur hexafluoride produced using the formula: mass = moles x molar mass. So, mass of SF6 = 0.025 moles x 146 g/mol = 3.65 g.