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hjlf
3 years ago
10

What's the difference between cracking and pyrolysis?

Chemistry
2 answers:
scoundrel [369]3 years ago
5 0
The difference between Cracking and Pyrolysis in the former is the process of whereby complex organic molecules such as kerogen or long chain hydrocarbon are broken into a simpler molecule while the later is a thermochemical decomposition of organic material at elevated temperature in the absence of oxygen.
boyakko [2]3 years ago
5 0
The difference between cracking and pyrolysis is that cracking is the breakdown of large organic compounds by use of a catalyst and low temperatures to form fewer different compounds. In Pyrolysis, it's the decomposition of a compound on heating in absence of air.
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HELP ASAP 20 POINTS
Colt1911 [192]

Solubility of a compound in water can be referred to as the amount of the compound that can be dissolved in 1 L of the solvent (water) at any given temperature. Solubility of a compound can be expressed in the units of g/L or mg/L.

Given that the solubility of calcium carbonate in water = 14 mg/L

We have to calculate the volume of water that can dissolve 11 g of calcium carbonate.

Converting 11 g calcium carbonate to mg:

11g *\frac{1000mg}{1g} =11,000 mg

Volume of water that would dissolve 11000 mg calcium carbonate

                             = 11000 mg CaCO_{3}*\frac{1L}{14 mg}

                             =785.7 L

Rounding the volume 785.7 L to two significant figures, we get 790 L water.

Therefore, we would need 790 L water to completely dissolve 11 g of calcium carbonate.

4 0
3 years ago
How many control(s) are in an experiment
weqwewe [10]
You can have as many controls as necessary, But they must remain equal at all times in order to get the most accurate results
6 0
3 years ago
Three moles of oxygen gas is stored in a 2.5-liter container at 35°C. What is the pressure of this gas?
nadezda [96]

Answer:

The pressure of the gas is 30.3072 atm.

Explanation:

An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar constant of the gases:

P * V = n * R * T

In this case:

  • P= ?
  • V= 2.5 L
  • n= 3 moles
  • R= 0.082 \frac{atm*L}{mol*K}
  • T= 35 C= 308 K (being 0 C= 273 K)

Replacing:

P* 2.5 L= 3 moles* 0.082 \frac{atm*L}{mol*K} *308 K

Solving:

P=\frac{ 3 moles* 0.082 \frac{atm*L}{mol*K} *308 K}{2.5 L}

P= 30.3072 atm

<u><em>The pressure of the gas is 30.3072 atm.</em></u>

4 0
3 years ago
Explain why the number of neutrons is not a factor in determining the charge of an ion.
Delvig [45]

Answer:

neutrons have a neutral charge, not positive or negative, therefore they won’t effect the charge in any way

Explanation:

8 0
3 years ago
When 25.0 ml of 0.500 m h2so4 is added to 25.0 ml of 1.00 m koh in a coffee-cup calorimeter at 23.50°c, the temperature rises to
AlladinOne [14]

The chemical reaction that occurs between the given substances is a neutralization reaction as shown below :

 

H_2SO_4 + 2KOH -> K_2SO_4 + 2H_2O

<span>1 mol            2 mol      1 mol           2 mol </span>

 

<span>The number of moles of the given substances  is calculated as shown : </span>

Number of moles of H_2SO_4 = 25.0 mL x 0.50 M = 12.5 millimoles

Number of moles of KOH = 25.0 mL x 1.00 M = 25.0 millimoles

 

As 1 mol of sulfuric acid reacts with 2 mol of KOH to give 2 mol of water, 12.5 millimoles of sulfuric acid completely reacts with 25.0 millimoles of KOH to give 25.0 millimoles of water.

Total volume of the solution = 25.0 mL + 25.0 mL = 50.0 mL.

Density of water is 1 g/mL. Use this to calculate the mass of the solution.

<span>Mass of the solution – 50.0 mL x 1 g/mL = 50.0  </span>

The specific heat of water is 4.184 J/gK. The temperature of the solution is increased from 23.5 degrees Celsius to 30.17 degrees Celsius.

The amount of heat released = 4.184 J/gK x 50.0 g x (30.17C – 23.50C) 1395 J

 

The amount of heat released per one mole of water formed can be calculated as shown :

The amount of heat released for formation of mole water = 1395 J / (25.0 m mol x 1mol/1000 m mol)

= 55,800 J

<span> </span>

8 0
3 years ago
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