If 3.50 mol of Fe reacts with 3.00 mol of oxygen in the following reaction: 4 Fe

Question

If 3.50 mol of Fe reacts with 3.00 mol of oxygen in the following reaction: 4 Fe(s) + 3 O2(g) 2 Fe2O3(s) Which of the following statements is correct? If 3.50 mol of Fe reacts with 3.00 mol of oxygen in the following reaction: 4 Fe(s) + 3 O2(g) 2 Fe2O3(s) Which of the following statements is correct?

a)Fe is the limiting reactant and 1.75 mol of product can be produced.

b)O2 is the limiting reactant and 2.00 mol of product can be produced.

c)Fe is the excess reactant and 1.75 mol of product can be produced.

d)O2 is the excess reactant and 2.00 mol of product can be produced.

Explanation / Answer

correct statement :

a) Fe is the limiting reactant and 1.75 mol of product can be produced

4 Fe(s) + 3 O2(g) ---------------> 2 Fe2O3(s)

   4            3                                       2 mol

3.50      3.0                                        ??

here limting reactant is Fe. becuause moles ration of Fe (3.50 / 4 = 0.875) is less than the O2 (3/3 = 1).

4 mol Fe   ------------> 2 mol Fe2O3

3.50 mol Fe       ----------> ??

moles of Fe2O3 formed = 3.50 x 2 / 4 = 1.75 mol

product formed = 1.75 mol

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