Consider the balanced chemical equation

(a) How many grams of CO could be produced from 10.0 g of PF₃, excess Fe(CO)₅, and excess H₂?

(b) How many grams of CO could be produced from 5.0 moles of Fe(CO)₅, 8.0 moles of PF₃, and 6.0 moles of H₂?

(c) How many moles of CO could be produced from 25.0 g of Fe(CO)₅, 10.0 g of PF₃, and excess H₂?

(d) The density of hydrogen gas at room temperature and atmospheric pressure is 0.0820 g/L. When 5.00 L of hydrogen gas at room temperature and atmospheric pressure is mixed with excess Fe(CO)₅ and excess PF₃, the mass of CO collected is 13.5 g. What is the theoretical yield (in grams) and the percent yield of CO?

Transcribed Image Text:

Fe(CO)5(s) +2 PF3(1)+H₂(g) → Fe(CO)2(PF3)2H2(s)+3 CO(g)