Question

In the reaction FeCl2 + 2NaOH ->Fe(OH)2(s) + 2NaCl, if 6 moles of FeCl2 are added to 6 moles of Na0H, how many moles of NaOH would be used up in the reaction? - Apex
A. 3
B. 6
C. 2
D. 1

Answer 1

Answer:

Correct answer is 3 Apex

Explanation:

Answer 2

Answer : The correct option is, (B) 6 mole

Explanation :

Given moles of $FeCl_2$ = 6 moles

Given moles of $NaOH$ = 6 moles

First we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

$FeCl_2+2NaOH\rightarrow Fe(OH)_2+2NaCl$

From the given balanced reaction, we conclude that

As, 1 moles of $FeCl_2$ react with 2 moles of $NaOH$

So, 6 moles of $FeCl_2$ react with $\frac{2}{1}\times 6=12$ moles of $NaOH$

From this we conclude that, $FeCl_2$ is an excess reagent and $NaOH$ is a limiting reagent because the given moles are less than the required moles and it limits the formation of product.

Thus, the number of moles of NaOH used up in the reaction = Required moles of NaOH - Given moles of NaOH

The number of moles of NaOH used up in the reaction = 12 - 6 = 6 moles

Therefore, the number of moles of NaOH used up in the reaction will be, 60 moles