Question

What is the S% in Fe2(SO3)3? and how would I figure this out?

Answer 1

Answer:

27

Explanation:

My explanation is the pdf, I also included instructions on how to find the percent comp. Hope this helps!

08533c7aed30d95e5d3b49054d9bddcb.pdf

Answer 2

To find :

$\sf \: S\% \: in \: Fe_2(SO_3)_3$

Procedure :

• First of all we need to find molar mass of Fe2(SO3)3
• Then we need to find amount of Sulphur in Fe2(SO3)3
• Then we will find percentage of Sulphur

Solution :

➝ Molar mass of Fe2(SO3)3 = 2× Molar mass of Iron + 3× { Molar mass of Sulfur + 3× (Molar mass of oxygen) }

➝ Molar mass of Fe2(SO3)3 = (2×56) + 3×{ 32 + (3×16) }

➝ Molar mass of Fe2(SO3)3 = 112 + 3×( 32 + 48)

➝ Molar mass of Fe2(SO3)3 = 112 + 3×80

➝ Molar mass of Fe2(SO3)3 = 112 + 240

➝ Molar mass of Fe2(SO3)3 = 352 g/mol

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Now , we will find total amount of Sulfur,

➝ Mass of Sulfur in Fe2(SO3)3 = 3× molar mass of Sulfur

➝ Mass of Sulfur in Fe2(SO3)3 = 3×32 = 96 grams/mol

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$\sf \: Percentage \: of \: S \: in \: Fe_2(SO_3)_3\: = \: \dfrac{Mass \: of \: Sulfur \: in \: Fe_2(SO_3)_3}{Molar \: mass \: of \: Fe_2(SO_3)_3} \times 100 \\ \\ \sf \implies \: Percentage \: of \: S \: in \: Fe_2(SO_3)_3\: = \dfrac{96}{352} \times 100 \\ \\ \sf \implies \: Percentage \: of \: S \: in \: Fe_2(SO_3)_3\: = 0.27 \times 100 \\ \\ \sf \implies \: Percentage \: of \: S \: in \: Fe_2(SO_3)_3\: = \bold{27}$

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ANSWER :

S% in Fe2(SO3)3 = 27%