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2 years ago

What are the products of any combustion reaction involving a hydrocarbon

Chemistry

2 answers:

Vaselesa [24]2 years ago

7 0

Answer:

The products of the combustion of hydrocarbons are carbon dioxide and water. Many hydrocarbons are used as fuel because their combustion releases very large amounts of heat energy.

Explanation:

sweet [91]2 years ago

4 0

Answer:

<em><u>The products of the combustion of hydrocarbons are carbon dioxide and water. Many hydrocarbons are used as fuel because their combustion releases very large amounts of heat energy.</u></em>

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Which property makes the materials used in fiber optic cables so useful? (1 point)

faust18 [17]

The property makes the materials used in fiber optic cables is:

C. High density

<h3>Fiber optic cables:</h3>

They transfer data signals in the form of light and travel hundreds of miles significantly faster than those used in traditional electrical cables. Fiber is immune to electrical interference. There is no cross - talk between signals in different cables and no pickup of environmental noise. Information traveling inside the optical fiber is even immune to electromagnetic pulses generated by nuclear devices.

Thus, correct option is C.

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2 years ago

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What is the mass in grams of 2.0 moles of NO2

mote1985 [20]

Use your periodic table to get 1 mol. Look up the atomic masses. I'll round the numbers since every periodic table is different.

N = 14
O2 = 2 *16
Total = 30 grams / mol

Therefore 2 mols = twice as much = 60 grams.

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3 years ago

In general, how do I figure out the total charge the neutrons have together ?

Crazy boy [7]

In atom, each proton is a charge of +1

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3 years ago

Explain how to calculate the density of a regular shaped object such as a rectangular box.

belka [17]

The density of a regular shaped object such as a rectangular box is calculated as thus:

The amount of matter is its mass, and the space it takes up is its volume.

So therefore, to calculate the density of an object such as the a regular shaped one like a rectangular box;

Its density = mass / volume.

<h3>Derived quantities</h3>

These are physical quantities which are obtained from fundamental quantities. I'm order words, derived quantities are quantities which are obtained from the combination of of fundamental quantities either by addition, division or multiplication

Some few examples of derived quantities are as follows:

Density

Velocity
Upthrust
Volume
Acceleration

So therefore, the density of a regular shaped object such as a rectangular box is calculated as thus:

The amount of matter is its mass, and the space it takes up is its volume.

So therefore, to calculate the density of an object such as the a regular shaped one like a rectangular box;

Its density = mass / volume.

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1 year ago

A student in chemistry 150-02 weighed out 55.5 g of octane (C8H18) and allowed it to react with oxygen, O2. The products formed

Anni [7]

Answer:

Explanation:

Given data:

Mass of octane = 55.5 g

Balanced chemical equation = ?

Mass of oxygen required to react = ?

Mass of CO₂ for med = ?

Molecules of water produced = ?

Mass of octane required to produced 30.0 g of water = ?

Solution:

Chemical equation:

2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O

Mass of oxygen required to react = ?

Mass of octane = 55.0 g

Solution:

Number of moles of octane:

Number of moles = mass/ molar mass

Number of moles = 55.0 g/114.23 g/mol

Number of moles = 0.48 mol

Now we will compare the moles of octane with oxygen.

C₈H₁₈ : O₂

2 : 25

0.48 : 25/2×0.48 = 6 mol

Mass of oxygen required:

Mass = number of moles × molar mass

Mass = 6 mol × 32 g/mol

Mass = 192 g

Given data:

Mass of carbon dioxide produced = ?

Mass of octane = 55g

Solution:

Number of moles of octane:

Number of moles = mass/ molar mass

Number of moles = 55.0 g/114.23 g/mol

Number of moles = 0.48 mol

Now we will compare the moles of octane with CO₂.

C₈H₁₈ : CO₂

2 : 16

0.48 : 16/2×0.48 = 3.84 mol

Mass of CO₂ produced:

Mass = number of moles × molar mass

Mass = 3.84 mol × 44 g/mol

Mass = 168.96 g

Given data:

Molecules of water produced = ?

Mass of octane = 55g

Solution:

Number of moles of octane:

Number of moles = mass/ molar mass

Number of moles = 55.0 g/114.23 g/mol

Number of moles = 0.48 mol

Now we will compare the moles of octane with H₂O.

C₈H₁₈ : H₂O

2 : 18

0.48 : 18/2×0.48 = 4.32 mol

Number of molecules of water:

1 mol = 6.022× 10²³ molecules

4.32 mol × 6.022× 10²³ molecules/ 1 mol

26 × 10²³ molecules

Given data:

Mass of octane required = ?

Mass of water produced = 30 g

Solution:

Number of moles of water.

Number of moles = mass/ molar mass

Number of moles = 30 g/ 18 gmol

Number of moles = 1.67 mol

Now we will compare the moles of water and octane from balance chemical equation:

2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O

H₂O : C₈H₁₈

18 : 2

1.67 : 2/18×1.67 = 0.185 mol

Mass of octane:

Mass = number of moles ×molar mass

Mass = 0.185 × 114.23 g/mol

Mass = 21.13 g

5 0

3 years ago