Question

When FeCl, is ignited in an atmosphere of pure oxygen, the following reaction takes place-
4FeCl (s) + 30,() - 2Fe,0,($)+ 6C1,(g)
If 3 moles of FeCl, are ignited in the presence of 2 moles of O, gas, how much of which reagent is
present in excess and therefore, remains unreacted?
(A)0.33 mole FeCl, remains unreacted (B) 0.67 mole FeCl, remains unreacted
(C) 0.25 mole 0, remains unreacted (D) 0.50 mole O remains unreacted​

Answer 1

Answer:

When FeCl3 is ignited in an atmosphere of pure oxygen, this reaction takes place.

4FeCl3(s) + 3O2(g) → 2Fe2O3(s) + 6Cl2(g)

If 3.00 mol of FeCl3 are ignited in the presence of 2.00 mol of O 2 gas, how much of which reagent is present in excess and therefore remains unreacted?

a) 0.33 mol FeCl3 remains unreacted

b) 0.67 mol FeCl3 remains unreacted

c) 0.25 mol O2 remains unreacted

d) 0.50 mol O2 remains unreacted

Explanation: