Question

To produce 264g iron sulphide,96g sulphur is used. Calculate the amount of iron required.​

Answer 1

Answer :  168gm of Fe si required.

Explanation :

Reaction Fe + S = FeS

Mass of Fe + Mass of Sulphur = Mass of iron sulphide

Mass Fe + 96 = 264

Mass of Fe = 264 - 96 = 168gm

We can solve this using the mole concept too.

Number of moles of S =  mass / Molar mass = 96/32 = 3 mol.

As per the reaction 1 mole of Fe combines with 1 mole of  S to form 1 mol of  FeS.

Hence 3 moles of S will need 3 mole of Fe.

Hence mass of Fe = number of moles X Molar mass =  3 X 55.8 = 168gm  

Answer 2

Answer:

168 is the answer.

Explanation:

If a = solvent and b = solute. Then, a+b=c

Now, we know that here b= 96g sulpher and c = 264g iron sulphide.

Therefore, c-b=a. 264g-96g=168g.

So your answer is 168g.

Please mark me as brainliest...