Based on the balanced equation below, how many moles of SF6 can form from the combination of 6 moles of S and 15 moles of F2?

Explanation:

1. Gather all the information in one place.

            S + 3F₂ ⟶ SF₆

n/mol:   6    15

They have given us the amounts of two reactants and asked us to calculate the amount of product. This is a limiting reactant problem.

2. Calculate the moles of SF₆ you can obtain from each reactant

From S:

From F₂:

SF₆ is the limiting reactant, because it gives fewer moles ( 5 mol) of SF₆.

The reaction can form 5 mol of SF₆.

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2

the seeing the electronic configuration we can say that the element is fluorine.

fluorine is the most electronegative element in the periodic table.

but by only seeing the configuration we cannot say about its reactivity because we don't know if its configuration after excitation or by addition of electrons.

but if not then, it is the lightest halogen and exists as a highly toxic pale yellow diatomic gas at standard conditions. as the most electronegative element, it is extremely reactive: almost all other elements, including some noble gases, form compounds with fluorine.