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Firlakuza [10]
3 years ago
13

8. Zeolite is used to remove moisture from methane. A vertical column is filled with 1000.0 kg of dry zeolite. The zeolite has t

he capacity to hold 0.100 kg water/kg dry zeolite. Once the zeolite becomes saturated with moisture, it must be regenerated by heating. The inlet moisture content of the methane is 7.00% (by mass) and the outlet moisture content is 0.05% (by mass). How much methane (kg) will be produced before the zeolite must be regenerated
Chemistry
1 answer:
Natasha_Volkova [10]3 years ago
3 0

Answer:

Follows are the solution to this question:

Explanation:

Methane inlet humidity content of =7.00\%

Methane moisture outlet content =0.05\%

Zeolite absorption humidity = 6.95\%

Dry zeolite 1 kg will accommodate water= 0.1000 \ kg

One kilogram of Dry Zeolite will carry water from =0.1000\ kg

The water can contain 1000 kg of zeolite = 100 \ kg

Methane which would be made =\frac{100}{6.95\%}= 1,439 \ kg

That's why it will be producing 1439 kg of methane.

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Electrons exist in specified energy levels surrounding the nucleus.

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The reaction A + B → 2 C has the rate law rate = k[A][B]³. By what factor does the rate of reaction increase when [A] remains co
lawyer [7]

Answer:

8

Explanation:

To solve this question, we just need to put the new number into the equation. If [A] remain constant then that mean [A2]= [A1]. If B doubled, then that mean [B2]= 2[B2]. To find what factor does the rate of reaction increases, we need to divide the first reaction rate with the second. The calculation will be:

rate2/rate1= k[A2][B2]³     /     k[A1][B1]³

rate2/rate1= [A1][2B1]³      /     [A1][B1]³

rate2/rate1=  A1*8B1³       /     A1*B1³

rate2/rate1= 8/1= 8

The rate of reaction will be 8 times faster.

7 0
3 years ago
Explain how Beer’s law can be applied in food, drug or medical testing
KonstantinChe [14]
<h2>Answer with explanation:</h2>

<em><u>Beer's Law is described as if a light passes from a solution, the concentration of the solution is directly proportional to the  absorbance of light by that solution.</u></em>

Every element has a definite of absorbance of light.

In the testing of food, drugs or in medical testing, the light is passed from the sample.

Them transmitted light from these samples are measured. The difference between target light amount and transmitted light is the amount of absorbed light.

From this absorbed light value, we can identify an element in sample and its quantity.

Spectrophometry is based on this law.

8 0
3 years ago
If you were asked to convert 4.2 × 1022 atoms of aluminum to moles, which of the following should you use for the conversion?
gregori [183]
You should use Avogadro’s number for the conversion, because Avogadro’s Law states that there are 6.02 x 10^23 atoms per 1 mol of that substance.
4 0
3 years ago
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How much CO2 is produced from the combustion of a tank of propane C3H8? Assume the tank contains 9kgs of propane and the molecul
Zinaida [17]

<u>Answer:</u> The mass of carbon dioxide produced is 26.9 kg

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}      .....(1)

Given mass of propane = 9 kg = 9000 g    (Conversion factor:  1 kg = 1000 g)

Molar mass of propane = 44.1 g/mol

Putting values in equation 1, we get:

\text{Moles of propane}=\frac{9000g}{44.1g/mol}=204.08mol

The chemical equation for the combustion of propane follows:

C_3H_8+5O_2\rightarrow 3CO2+4H_2O

By Stoichiometry of the reaction:

1 mole of propane produces 3 moles of carbon dioxide.

So, 204.08 moles of propane will produce = \frac{3}{1}\times 204.08=612.24mol of carbon dioxide.

Now, calculating the mass of carbon dioxide by using equation 1, we get:

Molar mass of carbon dioxide = 44.01 g/mol

Moles of carbon dioxide = 612.24 moles

Putting values in equation 1, we get:

612.24mol=\frac{\text{Mass of carbon dioxide}}{44.01g/mol}\\\\\text{Mass of carbon dioxide}=(612.24mol\times 44.01g/mol)=26944.7g=26.9kg

Hence, the mass of carbon dioxide produced is 26.9 kg

3 0
3 years ago
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