Question

If Iron is in Excess then production of 3 moles of Ferric Chloride requires?
A.319.5g of Cl
B.213g of Cl
C.106.5g of Cl
D.71g of Cl
(correct answer is "A" how? plz help me solve it)​

Answer 1

Answer:

Consider the reaction:

(1) FeCl3 (aq) + 3NaOH (aq) → Fe(OH)3 (s) + 3NaCl (aq)

This balanced equation tells us: one mole of iron(III) chloride reacts with three moles of sodium

hydroxide to produce one mole of iron(III) hydroxide and three moles of sodium chloride.

Several mole ratio fractions are possible:

3 mol/NaOH or 1 mol FeCl3/3 mol NaCl

or or and others

1 mol FeCl3 1 mol Fe(OH)3 1 mol FeCl3

You recognize these as conversion factors. The first relates moles of the two reactants; the

second and third relate one of the reactants to one of the products.

No matter how much of each reactant there is to start with they will react only in the ratio of 1

mol FeCl3 / 3 mol NaOH. If exactly one mole of FeCl3 and three moles of NaOH are brought

together, both reactants will be completely consumed. If one mole of FeCl3 and five moles of

NaOH are brought together, only three moles of the NaOH will react; two moles of NaOH will be

left unreacted. If three moles of FeCl3 and three moles of NaOH are brought together, two

moles of FeCl3 will remain unreacted.

Answer 2

Answer:

Explanation:

Fe + 3Cl ==> FeCl3

Now from eq

1 mole FeCl3 requires 3 moles of Cl

So 3 moles will require how much moles of Cl? (Just cross multiple)

moles of Cl = 3×3 =9 moles.

We know

Moles= mass / molar mass

Mass= moles × molar mass

= 9 × 35.5( molar mass of Cl)

= 319.5 g