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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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True or false in a chemical reaction some of the atoms will be changed into different type of atoms​
Anika [276]

Answer:

It's false

Explanation:

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To the nearest 0.5 mL, what is<br> the water volume in the<br> graduated cylinder?<br> mL?
AnnZ [28]

Answer:

14cm^3

Explanation:

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A crate holds 20 boxes of sewing supplies. Each box contains 8 spools of thread. Each spool has 250 meters of thread wrapped aro
exis [7]

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1 year ago
The pH of a 1.0M solution of butanoic acid HC4H7O2 is measured to be 2.41. Calculate the acid dissociation constant Ka of butano
Lubov Fominskaja [6]

Answer:

Ka = 1.52 E-5

Explanation:

  • CH3-(CH2)2-COOH ↔ CH3(CH2)2COO-  + H3O+

⇒ Ka = [H3O+][CH3)CH2)2COO-] / [CH3(CH2)2COOH]

mass balance:

⇒<em> C</em> CH3(CH2)2COOH = [CH3(CH2)2COO-] + [CH3(CH2)2COOH] = 1.0 M

charge balance:

⇒ [H3O+] = [CH3(CH2)2COO-]

⇒ Ka = [H3O+]²/(1 - [H3O+])

∴ pH = 2.41 = - Log [H3O+]

⇒ [H3O+] = 3.89 E-3 M

⇒ Ka = (3.89 E-3)² / ( 1 - 3.89 E-3 )

⇒ Ka = 1.519 E-5

3 0
3 years ago
Since helium is lighter than air, it is difficult to measure the mass of a sample, so to find out the mass of helium in a birthd
d1i1m1o1n [39]

Answer:

0.7457 g is the mass of the helium gas.

Explanation:

Given:  

Pressure = 3.04 atm

Temperature = 25.0 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T₁ = (25.0 + 273.15) K = 298.15 K  

Volume = 1.50 L

Using ideal gas equation as:

PV=nRT

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

3.04 atm × 1.50 L = n × 0.0821 L.atm/K.mol × 298.15 K  

<u>⇒n = 0.1863 moles</u>

Molar mass of helium = 4.0026 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

0.1863\ mole= \frac{Mass}{4.0026\ g/mol}

Mass_{He}= 0.7457\ g

<u>0.7457 g is the mass of the helium gas. </u>

6 0
2 years ago
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