Question

how do you calculate the mass of iron that contains the same number of moles as the mass of sulfur you have been given (170g sulfur) - to set up a reaction between these elements to produce iron sulfide

Answer 1

The mass of iron is 296.70 grams

Explanation:

Given information

Mass of sulfur = 170 g

Let x represents the mass of iron

The next step is to write a balanced chemical equation for the reaction

`Fe_((s))+S_((s))\text{ }\rightarrow FeS_((s))`

From the balanced chemical equation above, you will see that one mole of sulfur reacts with one mole of iron to produce one mole of iron sulfide

The next thing is to find the mole of sulfur using the below formula

`\text{mole = }\frac{\text{ reacting mass}}{\text{molar mass}}`

According to the periodic table, the molar mass of sulfur is 32 g/mol

`\begin{gathered} \text{mole = }(170)/(32) \\ \text{mole = 5.3125 moles} \end{gathered}`

To find the mole of iron, we will be using a stoichiometry ratio

`\begin{gathered} 1\text{ moles of sulfur = 1 mole of iron} \\ 5.3125\text{ moles of sulfur = x moles of iron} \\ \text{Mathematically,} \\ 1\text{ = 1} \\ 5.3125\text{ = x} \\ \text{cross multiply} \\ 1\cdot\text{ x =5.3125 }\cdot\text{ 1} \\ x\text{ = 5}.3125\text{ moles} \end{gathered}`

Therefore, the moles of iron is 5.3125 moles

The next step is to find the mass of iron using the below formula

`\text{Mole = }\frac{\text{ reacting mass}}{\text{molar mass}}`

From the periodic table, the molar mass of iron is 55.85g/mol

Let x be the mass of iron

`\begin{gathered} 5.3125\text{ = }(x)/(55.85) \\ \text{cross multiply} \\ x\text{ = 5.3125 }\cdot\text{ 55.85} \\ x\text{ = }296.70g \end{gathered}`

Therefore, the mass of iron is 296.70 grams