A student carries out the following reaction: 2 Fe (s) + 3 S (g) → Fe2S3 (s). The student determines that 2.67 moles of iron (III) sulfide were produced, resulting in a percent yield of 63%. Prior to conducting the reaction of iron with sulfur, the student produced the gaseous sulfur that was used via heating solid sulfur in a syringe.

S8 (s) + heat → 8 S (g)

Assume all of the sulfur was converted to the gaseous form, and the entirety of the gaseous sulfur was used in the reaction. What mass of solid sulfur was used in producing the gaseous sulfur?

A.
408 g

B.
913 g

C.
484 g

D.
8547 g