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2 years ago

Crude oil is a mixture of many different chemical compounds.

Chemistry

1 answer:

evablogger [386]2 years ago

6 0

Answer:

092) Icosane

093) Ethene

Explanation:

092) The given compounds are;

Decane C₁₀H₂₂; Viscosity = 0.850 mPa·s (25°C)

Ethene C₂H₄ (gas); Viscocity ≈ 0.01038 m

Icosane C₂₀H₄₂; Solid at room temperature

Methane CH₄; gas at room temperature

The viscosity of the given carbon and hydrogen compounds is observed to increase with their molar masses

Therefore, icosane, which is a solid at room temperature, has the highest viscosity (resistance to deformation) out of the given compounds

093) Polymers are made from monomer alkene units, therefore, ethene, which is the only alkene among the given compounds can be used to produce a polymer

Polyethene is formed by the polymerization of ethene whereby molecules of ethene are joined together to form poly(ethene)

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A shampoo has a pH of 8.59. What is the [H3O+] in the shampoo?

Cerrena [4.2K]

Answer:

2.57 e-9

Explanation:

The formula is H3O=10^-Ph

10^-8.59=2.57 e-9

6 0

2 years ago

How many moles of mercury, Hg, are there in 1.30 x 10^7 atoms of murcury? PLEASE HELP, IT'S URGENT! Thank you! (:

vodka [1.7K]

1 mole Hg ---------------- 6.02x10²³ atoms
?? ------------------------- 1.30 x10⁷ atoms

1.30x10⁷ x 1 / 6.02x10²³ =

= 1.30x10⁷ / 6.02x10²³ => 2.159x10⁻¹⁷ moles

hope this helps!

7 0

3 years ago

What is the volume of 1.56 kg of a compound whose molar mass is 81.86 g/mole and whose density is 41.2 g/ml?

hjlf

Answer:

v = 37.9 ml

Explanation:

Given data:

Mass of compound = 1.56 kg

Density = 41.2 g/ml

Volume of compound = ?

Solution:

First of all we will convert the mass into g.

1.56 ×1000 = 1560 g

Formula:

D=m/v

D= density

m=mass

V=volume

v = m/d

v = 1560 g / 41.2 g/ml

v = 37.9 ml

7 0

3 years ago

What expression approximates the volume of O2 consumed, measure at STP, when 55 g of Al reacts completely with excess O2?2 Al(s)

Genrish500 [490]

Answer:

34.28 L ( 1.5*22.4 L)

Explanation:

Calculation of the moles of aluminum as:-

Mass = 55 g

Molar mass of aluminum = 26.981539 g/mol

The formula for the calculation of moles is shown below:

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

Thus,

$Moles= \frac{55\ g}{26.981539\ g/mol}$

$Moles= 2.0384\ mol$

According to the reaction:-

$4Al+3O_2\rightarrow 2Al_2O_3$

4 moles of aluminum react with 3 moles of oxygen gas

1 mole of aluminum react with $\frac{3}{4}$ moles of oxygen gas

2.0384 moles of aluminum react with $\frac{3}{4}\times 2.0384$ moles of oxygen gas

Moles of oxygen gas = 1.5288 moles

At STP,

Pressure = 1 atm

Temperature = 273.15 K

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:

1 atm × V = 1.5288 mol × 0.0821 L.atm/K.mol × 273.15 K

⇒V = 34.28 L ( 1.5*22.4 L)

7 0

3 years ago

Can someone plz help me? :(

Snezhnost [94]

Answer:

The answer is a. I learned that they can multiply by using your cells

6 0

2 years ago

Read 2 more answers