Question

1.Calculate the number of moles of SO₃ formed when 14.0 moles of sulfur dioxide are mixed with 8.0 moles of oxygen.

2. a) Set up the ICE table for the reaction P₄ + Cl₂ --> 4PCl₅ . Initially 84.5 g of phosphorus are mixed with an amount of chlorine. In the Change row calculate the mass of chlorine required to completely react with 84.5 g of phosphorus.

b) Calculate the mass of PCl₅ produced when 84.5 g of phosphorus combines with the amount of chlorine calculated in part a.

Answer 1

1)

The balanced equation for reaction taking place is:

2 SO2   +   O2   —> 2 SO3

from reaction, 2 mol of SO2 will react with 1 mol of O2

So, 14 moles of SO2 will react with 7.0 mol of O2

O2 will still remain

So,SO2 is limiting reagent

we will use SO2 in our further calculations

from balanced equation above:

moles of SO3 formed = moles of SO2 reacted

= 14.0 mole

Answer: 14.0 mole

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