2 Points

What is one chemical reaction that begins with petroleum as a starting material

emmasim [6.3K]

Answer:

Thermal decomposition or cracking

Explanation:

Petroleum is a mixture of hydrocarbons which are usually formed naturally. Petroleum undergo a host of chemical reactions. One of such is thermal decomposition or cracking.

Cracking is used in the petroleum industry to covert heavy fractions to more useful lighter ones.

When petroleum is subjected to high temperature and pressure, and in the presence of catalyst, the long chain type of petroleum will decompose into more useful smaller and lighter molecules.

Example is given below:

C₁₅H₃₂ → C₈H₁₈ + C₃H₆ + 2C₂H₄

6 0

4 years ago

The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most rem

son4ous [18]

Answer:

10 kg Al(OH)₃

Explanation:

There is some info missing. I think this is the original question.

The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of 19th-century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today.

In the first step, aluminum hydroxide reacts to form alumina (Al₂O₃) and water: 2 Al(OH)₃(s) → Al₂O₃(s) + 3H₂O(g). In the second step, alumina (Al₂O₃ and carbon react to form aluminum and carbon dioxide: 2Al₂O₃(s)+3C(s)→4Al(s)+3CO₂(g). Suppose the yield of the first step is 63% and the yield of the second step is 89%.

Calculate the mass of aluminum hydroxide required to make 2.0 kg of aluminum. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.

Let's consider the 2 steps in the synthesis of Al.

Step 1: 2 Al(OH)₃(s) → Al₂O₃(s) + 3 H₂O(g)

Step 2: 2 Al₂O₃(s) + 3 C(s) → 4 Al(s) + 3 CO₂(g)

In Step 2, the percent yield of Al is 89% and the real yield is 2.0 kg. The theoretical yield is:

2.0 kg (R) × (100 kg (T) / 89 kg (R)) = 2.2 kg = 2.2 × 10³ g

In Step 2, the mass of Al is 4 × 26.98 g = 107.9 g and the mass of Al₂O₃ is 2 × 101.96 g = 203.92g. The mass of Al₂O₃ that produced 2.2 × 10³ g of Al is:

2.2 × 10³ g Al × (203.92g Al₂O₃ / 107.9 g Al) = 4.2 × 10³ g Al₂O₃

In Step 1, the percent yield of Al₂O₃ is 63% and the real yield is 4.2 × 10³ g. The theoretical yield is:

4.2 × 10³ g (R) × (100 g (T)/ 63 g (R)) = 6.7 × 10³ g

In Step 1, the mass of Al₂O₃ is 101.96 g and the mass of Al(OH)₃ is 2 × 78.00 g = 156.0 g. The mass of Al(OH)₃ that produced 6.7 × 10³ g of Al₂O₃ is:

6.7 × 10³ g Al₂O₃ × (156.0 g Al(OH)₃ / 101.96 g Al₂O₃) = 1.0 × 10⁴ g Al(OH)₃ = 10 kg Al(OH)₃

7 0

4 years ago

How could a synthetic material such as Acegram affect society?

pantera1 [17]

Explanation:

Synthetic fiber or synthetic fibre (in British English; see spelling differences) are fibers made by humans through chemical synthesis, as opposed to natural fibers that are directly derived from living organisms. They are the result of extensive research by scientists to improve upon naturally occurring animal and plant fibers. In general, synthetic fibers are created by extruding fiber-forming materials through spinnerets, forming a fiber. These are called synthetic or artificial fibers. Synthetic fibers are created by a process known as polymerization, which involves combining monomers to make a long chain or polymer. The word polymer comes from a Greek prefix "poly" which means "many" and suffix "mer" which means "single units". (Note: each single unit of a polymer is called a monomer). There are two types of polymerization: linear polymerization and cross-linked polymerization.

8 0

3 years ago

If 1.8 L of water is added to 2.5 L of a 7.0 M KOH solution, what is the molarity of the new solution?

e-lub [12.9K]

Molarity= (number of moles of that substance) / (Volume of solution in litres)

7= (number of moles of HCl) / 0.05

Thus,

Number of moles of HCl = 7 x 0.05 = 0.35

The number of moles of HCl will remain unchanged.

Now, for new solution,

0.35= 0.35 / (New volume of solution in litres)

Thus,

New volume = 1 litre

Thus, amount of water added = 1- 0.05 litre = 5.0 M

6 0

3 years ago

What volume of 0.05 mol/L HCl is required to react with 5.00g of manganese dioxide according to this equation?

adell [148]

217 ml of 0.05 M HCl will be required to react with 5 gm of MnO2 according to the equation given.

Explanation:

The balanced chemical equation is given as:

4HCl(aq) + MnO2(s) → 2H2O(l) + MnCl2(aq) + Cl2(g)

This shows that 4 moles of HCl reacts with 1 mole of MnO2

the mass of Manganese oxide is given as 5 grams

molar mass of MnO2 = 86.93 grams/mole

number of moles of MnO2 is given by

number of moles = $\frac{mass}{atomic mass of one mole}$

number of moles= $\frac{5}{86.93}$

= 0.0575 moles of MnO2

From the equation:

4 moles of HCl reacts with 1 mole of MnO2

x moles of HCl reacts with $\frac{0.0575}{x}$ moles of MnO2

$\frac{1}{4}$ = $\frac{0.0575}{x}$

= 0.23 moles of HCl will react

atomic mass of HCl = 36.46 Grams/mole

mass = 0.23 x 36.46

= 8.3858 grams.of HCl

molarity of HCl = $\frac{number of moles}{volume in liters}$

volume is 1 litre

so molarity is 0.23 M

Using the formula

M1V1 = M2V2

0.05 x 1 = 0.23 X x

x = 0.217 litre

so 217 ml of 0.05 M HCl will be required to react with 5 gm of MnO2.

4 0

3 years ago