Chemistry, 18.03.2020 20:05 Jadaaaaaaan

Determine the volume of SO2 (at STP) formed from the reaction of 96.7 g of FeS2 and 55.0 L of O2 (at 398 K and 1.20 atm). The molar mass of FeS2 is 119.99 g/mol. 4 FeS2(s) + 11 O2(g) → 2 Fe2O3(s) + 8 SO2(g)

Answers: 3

Show answers

Answers

Answer from: tbair5417

The volume of SO₂ formed from the reaction at STP is 32.92 L

From the question,

We are to determine the volume of SO₂ formed from the reaction

The given balanced chemical equation for the reaction is

4FeS₂(s) + 11O₂(g) → 2Fe₂O₃(s) + 8SO₂(g)

This means,

4 moles of FeS₂ reacts with 11 moles of oxygen to produce 2 moles of Fe₂O₃ and 8 moles of SO₂

First, we will determine the number of moles of each reactant present

For FeS₂

Mass = 96.7 g

From the formula

$Number\ of\ moles =\frac{Mass}{Molar\ mass}$

Molar mass of FeS₂ = 119.99 g/mol

∴ Number of moles of FeS₂ present = $\frac{96.7}{119.99}$

Number of moles of FeS₂ present = 0.8059 mole

For O₂

Using the formula

PV = nRT

$n =\frac{PV}{RT}$

Putting the given parameters into the formula, we get

$n = \frac{1.2 \times 55.0}{0.08206 \times 398}$

$n = \frac{66}{32.65988}$

n = 2.0208 moles

Since,

4 moles of FeS₂ reacts with 11 moles of oxygen to produce 8 moles of SO₂

Then,

$\frac{2.0208 \times 4}{11}$ moles of FeS₂ will react with 2.0208 moles of oxygen to produce $\frac{2.0208 \times 4}{11} \times 2$ moles of SO₂

That is,

0.7348 moles of FeS₂ will react with 2.0208 moles of oxygen to produce 1.4697 moles of SO₂

∴ Number of moles of SO₂ formed is 1.4697 moles

Now for the volume of SO₂ formed at STP

Since

1 mole of a gas has a volume of 22.4 L at STP

Then

1.4697 moles of the SO₂ will have a volume of 1.4697 × 22.4 L

1.4697 × 22.4 L = 32.92L

Hence, the volume of SO₂ formed from the reaction at STP is 32.92 L

Learn more here: link

Answer from: deedee363

32.9 Liters

Explanation:

To calculate the moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}$

1. moles of $FeS_2=\frac{96.7g}{119.99g/mol}=0.806mol$

2. moles of O_2

PV=nRT

P = pressure of the gas = 1.20 atm

R = Gas constant = $0.0821\text{ L atm }mol^{-1}K^{-1}$

T = temperature of the gas = 398K

$1.20\times 55.0=n\times 0.0821\times 398$

n=2.02

$4FeS_2(s)+11O_2(g)\rightarrow 2Fe_2O_3(s)+8SO_2(g)$

According to stoichiometry:

11 moles of oxygen reacts with 4 moles of FeS_2

Thus 2.02 moles of oxygen reacts with = $\frac{4}{11}\times 2.02=0.73$ moles of FeS_2

Thus oxygen acts as limiting reagent and FeS_2 is excess reagent.

As 11 moles of oxygen gives = 8 moles of SO_2

2.02 moles of oxygen gives = $\frac{8}{11}\times 2.02=1.47$ moles of SO_2

PV=nRT

P = pressure of the gas = 1 atm (at STP)

R = Gas constant = $0.0821\text{ L atm }mol^{-1}K^{-1}$

T = temperature of the gas = 273K (at STP)

$1\times V=1.47\times 0.0821\times 273$

V=32.9L

Thus volume of SO_2 (at STP) formed from the reaction is 32.9 L

Answer from: Quest

ljjjljlj kjlk,ljym jlyu; jm; l mumytj

Answer from: Quest

if you mean hydrogen and oxygen then water is the product

Another question on Chemistry

Chemistry, 22.06.2019 00:30

Asolution of sodium hydroxide was titrated against a solution of sulfuric acid. how many moles of sodium hydroxide would react with 1 mole of sulfuric acid?

Answers: 2

Answer

Chemistry, 22.06.2019 05:30

Astudent carefully transfers 30 g of water and 30 g of alcohol in a glass tube, forming two layers and filling the tube completely. after sealing the tube, the student mixes the solutions, and notices a bubble that forms in the tube. what is the mass of the contents in the glass tube after mixing?

Answers: 2

Answer

Chemistry, 22.06.2019 07:30

In the particles are arranged in a regular, repeating pattern. a)a crystalline liquid b)a crystalline solid c)all gases d)all solids

Answers: 2

Answer

Chemistry, 22.06.2019 12:00

What is the subscript for oxygen in its molecular formula

Answers: 1

Answer

You know the right answer?

Determine the volume of SO2 (at STP) formed from the reaction of 96.7 g of FeS2 and 55.0 L of O2 (at...