Question

Need some help -

PCl5 can be produced by the reaction of phosphorus trichloride with excess chlorine as follows: PCl3 + Cl2 → PCl5

If the actual yield is 127 g of PCl5 and the percent yield is 84.8%, what mass of PCl3 must be used? Hint: Use actual yield and percent yield to find theoretical yield and proceed from there.

a. 150 g

b. 98.8 g

c.108 g

d.83.8 g

e.71.1 g

2. If the reaction N₂ + 3 H₂ → 2 NH₃ is carried out using 1.40 g of N₂ and 0.400 g of H₂, what mass of excess reactant will remain?

a. 0.200 g N₂

b. 1.00 g N₂

c. Both reactants will be completely consumed

d. 0.100 g H₂

e.0.300 g H₂

_3. How many moles of bromine will react with 0.0500 mole of C₂H₂ in the reaction C₂H₄ + Br₂ → C₂H₄Br₂?

a. 0.186 mol

b. 2.00 mol

c. 0.0250 mol

d. 0.100 mol

e. 0.0500 mol