Tin fluoride, SnF2, is used in some toothpastes. It is made by the reaction of tin with hydrogen fluoride according to the following equation: Sn(s) + 2HF(g) --> SnF2(s) +H2(g). If a toothpaste manufacturer reacts 30.00 of HF with enough tin, how many grams of SnF2 can they expect to get? Please show your work or how you got the answer, I really need it.

Mass of SnF2 : 117.53 g

Given

Reaction

Sn(s) + 2HF(g) --> SnF2(s) +H2(g).

30 g of HF

Required

mass of SnF2

Solution

mol HF (MW= 20 g/mol) :

= mass : MW

= 30 : 20

= 1.5

From the equation, mol ratio of HF : SnF2 = 2 : 1, so mol SnF2 :

=1/2 x mol HF

= 1/2 x 1.5

= 0.75

mass SnF2(MW=156.71 g/mol) :

=mol x MW

= 0.75 x 156.71

= 117.53 g

elements make up everything, and they combine to make compounds.

the answer is c