Question

Boron trifluoride reacts with hydrogen according to the following balanced equation:
2 BF3 (g) + 3 H2 (g) → 2 B (s) + 6 HF (g)
Suppose 40.00 grams of BF3 are mixed with 5.00 grams of H2.
Identify the limiting reactant.
Calculate the mass of HF generated.
Calculate the mass of excess reactant that remains when the reaction is complete.
When this reaction is performed in the laboratory, the percent yield of HF is 72.6%. What was the experimental yield of HF?

Answer 1

@supie

Answer 2

This is Chemistry idk it \[2 BF3 (g) + 3 H2 (g) → 2 B (s) + 6 HF (g)\] I think thay have to do something with that but idrk