Tin undergoes a synthesis reaction with hydrogen fluoride according to the
chemical equation below. How many grams of SnF2, are produced from the
reaction of 30.00 g HF with tin?

117.5 g of SnF₂ can be produced

Explanation:

Let's think the reaction:

Reactants are Sn and HF. Therefore the products are SnF₂ and H₂.

It is a redox reaction.

The equation is: Sn(s) + 2HF(g) → SnF₂(g) + H₂(g)

We convert the mass of the fluoride to moles

30 g . 1mol / 20g/mol = 1.5 moles of HF

By stoichiometry we produce 1 mol of SnF₂ with 2 moles of HF. Let's make a rule of three:

If 2 moles of HF can make 1 mol of SnF₂

Then, 1.5 moles of HF must produce (1.5 . 1) /2 = 0.75 moles of SnF₂

We convert the moles to mass  →  0.75 mol . 156.71 g /1mol = 117.5 g

the answer would be c

i think slash and