Sulfuric acid is probably the most important industrial chemical because it is used in so many industrial processes to produce or purify other chemicals. It can be produced by a three step process. First, sulfur is burned in air to give sulfur dioxide. Second, the sulfur dioxide is converted to sulfur trioxide by passing the sulfur dioxide over a catalyst in the presence of oxygen at a high temperature. Third, the sulfur trioxide is reacted with water to produce sulfuric acid. If the three steps gave yields as listed below and you start with 1.00 x 103 kg of sulfur (assume other reagents are in excess), how much sulfuric acid can be produced?

The stoichiometry between the sulfur and sulfur dioxide is 1:1, thus, multiplying it by their molar masses, we can obtain the relationship between masses. The molar mass of sulfur is 32.065 g/mol, and of sulfur dioxide is 64.066 g/mol, thus:

1*32.065 --- 1*64.066

32.065 g of S ------ 64.066 g of SO2

1.00x10³ kg of S --- x

By a simple direct rule of three:

32.065x = 64066

x = 2.00x10³ kg of SO2

Bceause the yield is 92.5%, the mass formed of SO2 that follows for the second step is:

m = 0.925*2.00x10³

m = 1.85x10³ kg

Step 2

2SO2 + O2 ⟶ 2SO3

Now, two moles of SO2 produces 2 moles of SO3, thus, the stoichiometry is still 1:1, and the molar mass of SO3 is 80.066 g/mol, thus the mass relationship is:

64.066 g of SO2--------- 80.066 g of SO3

1.85x10³ kg of SO2 ----- x

By a simple direct rule of three

64.066x = 148122.1

x = 2.31x10³ kg

Because the yield is 72.6%, thus the mass of SO3 that is produced and follows for the last step is:

m = 0.726*2.31x10³

m = 1.68x10³ kg of SO3

Step 3

SO3 + H2O ⟶ H2SO4

Now, the stoichiometry os SO3 and H2SO4 is 1:1, and the molar mass of the sulfuric acid is 98.079 g/mol, so:

80.066 g of SO3 ------- 98.079 g of H2SO4

1.68x10³ kg of SO3 --- x

By a simple direct rule of three

80.066x =164772.72

x = 2.06x10³ kg

Because the yield is 98.2%, the mass of sulfuric acid produced is:

m = 0.982*2.06x10³

m = 2.02x10³ kg of H2SO4

ajeigbeibraheem ajeigbeibraheem · Answer 2 · 2022-01-20T10:51:02+01:00

The amount of sulfuric acid that is produced from the yields of the reaction is 2020 kg of Sulfuric acid.

What is Sulfuric acid?

Sulfuric acid is presumably the most significant industrial chemical due to the fact that it is utilized in so many industrial processes to manufacture or purify other chemicals.

The production of sulphuric acid occurs in a 3-step reaction process.

Burning of Sulfur in the air to produce sulfur dioxide.

[tex]\mathbf{S + O_2 \to SO_2}[/tex] 92.5%

Conversion of Sulfur dioxide to Sulfur trioxide

[tex]\mathbf{2SO_2 + O_2 \to 2SO_3 }[/tex]

The reaction of sulfur trioxide with water to produce sulfuric acid.

[tex]\mathbf{SO_3 + H_2O \to H_2SO_4}[/tex]

From the parameters given:

The initial mass of Sulphur is known to be = 1.00 × 10³ kg
= 1.00 × 10⁶ g

From the stochiometric standpoint, if 1 mole of sulfur = 32.065 grams;

Then, the moles of sulfur in 1.00 × 10⁶ g will be:

[tex]\mathbf{=\dfrac{10^6}{32.065}}[/tex]

= 31250 moles of sulfur

Now from this mole of sulfur, it is noted that 92.5% transform to SO2;

Thus, the amount of SO2 will be:

[tex]\mathbf{=31250 \times \dfrac{92.5}{100}} \\ \\ \mathbf{= 28906.25 \ mol \ of \ SO_2}[/tex]

In the second reaction; 28906.25 mol of SO2 will be transformed to SO3 with 72.6% yield.

Thus, the amount of SO3 will be:

[tex]\mathbf{=28906.25 \times \dfrac{72.6}{100}} \\ \\ \mathbf{= 20985.9375 \ mol \ of \ SO_3}[/tex]

In the third reaction; 20985.9375 mol of SO3 will be transformed to H2SO4 with 98.2% yield.

Thus, the amount of H2SO4 will be:

[tex]\mathbf{= 20985.9375 \times \dfrac{98.2}{100}} \\ \\ \mathbf{= 20608.19 \ mol \ of \ H2SO_4}[/tex]

Recall that:

1 mole of H2SO4 = 98 grams

Thus:

20608.19 mol of H2SO4 will be = 20608.19 × 98

= 2019602.62 g of H2SO4

Converting the answer to kilograms (kg), we have:

= 2019.60 kg

≅ 2020 kg of H2SO4

Learn more about sulfuric acid here:

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