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Snezhnost [94]
3 years ago
7

Sulfuric acid (H2SO4) is prepared commercially from elemental sulfur using the contact process. In a typical sequence of reactio

ns, the sulfur is first burned: S + O2 → SO2 , then it is converted to SO3 using a catalyst: 2 SO2 + O2 → 2 SO3 . The resulting SO3 is reacted with water to produce the desired product: SO3 + H2O → H2SO4 . How much sulfuric acid could be prepared from 83 moles of sulfur? Answer in units of g.
Chemistry
2 answers:
Elan Coil [88]3 years ago
8 0
I believe the end result is still 83 moles since there is never an amount of sulfur atoms added to the initial amount, but rather oxygen and water is repeatedly added to it. To find it's weight, first find the molar mass of H2SO4:

H2 + S + O4 = 2.00 + 32.1 + 64.0 = 98.1 g/mol

and mass = (98.1 g/mol)(83 mol) = 8142.3 g

rounded to 8.1 x 10^3 g assuming 100% yield?
saveliy_v [14]3 years ago
6 0

Answer:

8134gH_{2}SO_{4}

Explanation:

From the first reaction:

S+O_{2}=SO_{2}

Finding the number of moles using stoichiometry:

83molesS*\frac{1molSO_{2}}{1molS}=83molesSO_{2}

Using stoichiometry in the second reaction:

_{2}SO_{2}+O_{2}=_{2}SO_{3}

83molesSO_{2}*\frac{2molesSO_{3}}{2molesSO_{2}}=83molesSO_{3}

From the third reaction:

SO_{3}+H_{2}O=H_{2}SO_{4}

83molesSO_{3}*\frac{1molH_{2}SO_{4}}{1molSO_{3}}=83molesH_{2}SO_{4}

Finding the mass in grams of H_{2}SO_{4}:

83molesH_{2}SO_{4}*\frac{98gH_{2}SO_{4}}{1molH_{2}SO_{4}}=8134gH_{2}SO_{4}

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If the absorbance of a KMnO4 solution of unknown concentration is 0.633, calculate the concentration of KMnO4 in the solution.
solong [7]

The molar Concentration of KMnO₄ is 0.000219 M

Concentration is the abundance of a constituent divided by means of the overall extent of an aggregate. numerous styles of mathematical description may be outstanding: mass awareness, molar awareness, variety concentration, and quantity awareness.

y is absorbance

x is the molar concentration of KMnO_4

y = 4.84E + 03x - 2.26E - 01

0.833 = 4.84 * 10⁺⁰³ x - 2.26 * 10⁻¹

1.059 = 4.84 * 10⁺⁰³ x

X = 0.000219 M

Hence, The molar Concentration of KMnO₄ is 0.000219 M

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3 0
1 year ago
If 12.5 grams of strontium hydroxide is reacted with 150 mL of 3.5 M carbonic acid, identify the limiting reactant.
vesna_86 [32]

Answer:

Sr(OH)2

Explanation:

We'll begin by calculating the number of mole of carbonic acid in 150mL of 3.5 M carbonic acid solution. This is illustrated below:

Molarity = 3.5M

Volume = 150mL = 150/1000 = 0.15L

Mole of carbonic acid, H2CO3 =..?

Mole = Molarity x Volume

Mole of carbonic acid, H2CO3 = 3.5 x 0.15 = 0.525 mole.

Next, we shall convert 0.525 mole of carbonic acid, H2CO3 to grams.

Mole of H2CO3 = 0.525 mole

Molar mass of H2CO3 = (2x1) + 12 + (16x3) = 62g/mol.

Mass of H2CO3 =..?

Mass = mole x molar mass

Mass of H2CO3 = 0.525 x 62 = 32.55g

Next, we shall write the balanced equation for the reaction. This is given below:

Sr(OH)2 + H2CO3 → SrCO3 + 2H2O

Next, we shall determine the mass of Sr(OH)2 and H2CO3 that reacted from the balanced equation. This is illustrated below:

Molar mass of Sr(OH)2 = 88 + 2(16 + 1) = 88 + 2(17) = 122g/mol

Mass of Sr(OH)2 from the balanced equation = 1 x 122 = 122g

Molar mass of H2CO3 = (2x1) + 12 + (16x3) = 62g/mol.

Mass of H2CO3 from the balanced equation = 1 x 62 = 62g.

From the balanced equation above, 122g of Sr(OH)2 reacted with 62g of H2CO3.

Finally, we shall determine the limiting reactant as follow:

From the balanced equation above, 122g of Sr(OH)2 reacted with 62g of H2CO3.

Therefore, 12.5g of Sr(OH)2 will react with = (12.5 x 62)/122 = 6.35g.

We can see evidently from the calculations made above that it will take 6.35g out 32.55g of H2CO3 to react with 12.5g of Sr(OH)2. Therefore, Sr(OH)2 is the limiting reactant and H2CO3 is the excess reactant

5 0
3 years ago
Read 2 more answers
What is the empirical formula of a molecule containing 65.5% carbon, 5.5% hydrogen, and 29.0% oxygen
natta225 [31]
Carbon(C):
number of moles= mass/molar mass(Mr)
=65.5/12
=5.5 moles

Hydrogen(H):
number of moles=mass/molar mass (Mr)
=5.5/1
=5.5 moles

Oxygen (O):
number of moles = mass/molar mass (Mr)
=29.0/16
=1.8 moles

EF= lowest number of moles over each of the elements

So,
C= 5.5/1.8 = 3
H= 5.5/1.8 = 3
O= 1.8/1.8 = 1

Therefore Emperical formula= C3H3O
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Shalnov [3]

Answer:

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2 years ago
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