How would I solve this...........For each of the following unbalanced equations, calculate how many grams of each product would be produced by complete reaction of 12.5 g of the reactant indicated in boldface. Indicate clearly the mole ratio used for the conversion.

Question

How would I solve this...........For each of the following unbalanced equations, calculate how many grams of each product would be produced by complete reaction of 12.5 g of the reactant indicated in boldface. Indicate clearly the mole ratio used for the conversion.
 
 TiBr4(g) + H2 ⟶ Ti(s) + HBr(g)

oobleck · Answer

TiBr4 + 2H2 ⟶ Ti + 4HBr
Don't know which reactant is in bold face, but I assume it is the TiBr4. If so, you have 12.5/367.483 = 0.034 moles.

So now just calculate the mass of the products in the ratio shown.