Coal, oil, and natural gas A.
are renewable natural resources.

B.
are in very short supply for consumers.

C.
release carbon dioxide when they are burned.

D.
are clean fuels that contribute little to pollution.

Answer:

The correct answer is "Infrared light".

Explanation:

Infrared light, also known as infrared radiation, is a type of light that can no be seen but it can be felt from the heat that it generates. The spectrum of wavelengths that comprise the infrared light is given from 700 nanometers, which is the edge of visible red light, up to 1 millimeter of wavelength. Near-Infrared light is the one that can reach the highest temperature, reaching from 3000 to 5200 K. Therefore, a super-powerful flashlight heated up to 3600 K can be given off infrared light.

Answer:

A chemical reaction is the process by which a change takes place

Explanation:

A chemical reaction is a process by which one or more substances, called reactants, are transformed into one or more other substances with different properties, called products.

The bonds between the atoms that make up the reactants are broken. Then, the atoms rearrange themselves in another way, forming new bonds and giving rise to one or more different substances from the initial ones. So the atoms do not change, they remain the same, but it changes is the way they are linked together.

In short, chemical reactions are the process of arranging atoms and bonds when chemicals come into contact. The chemical properties change by altering the arrangement of the atoms in that substance.

So, a chemical reaction is the process by which a change takes place.

The heat required for the following two processes are:

a. 10.74 KJ

b. 83.92 KJ

Part a)

Given:

Mass (m) of ethanol = 100g

Heat of fusion, Hfus = 4.94 kJ/mol

To find:

Heat (Q) =?

Calculation for number of moles:

Mass of C₂H₅OH = 100g

Molar mass of C₂H₅OH = (2x12)+ (5x1) + 16 + 1 = 46g/mol

Number of Mole = Mass /Molar Mass

Number of mole (n) of C₂H₅OH = 100/46 = 2.174 moles.

Calculation for Heat of fusion:

Q = n x Hfus

Q = 2.174 mol x 4.94 kJ/mol

Q = 10.74KJ

Therefore, 10.74 KJ of heat is required to melt the ethanol.

Part b)

Given:

Mass of C₂H₅OH = 100g

Heat of vaporization, Hvap = 38.6 kJ/mol

To find:

Heat (Q) =?

Calculation for Heat of vaporization:

As calculated above, the number of mole in 100g of ethanol, C₂H₅OH is 2.174 moles.

The heat required to vaporize the ethanol can be obtained as follow:

Q = n x Hvap

Q = 2.174 mol x 38.6 kJ/mol

Q = 83.92 KJ

Therefore, 83.92 KJ of heat is required to vaporize the ethanol.

Find  more information about Heat of fusion here:

brainly.com/question/87248

Answer:

A. 10.74 KJ

B. 83.92 KJ

Explanation:

A. Data obtained from the question include the following:

Mass (m) of ethanol = 100g

Heat of fusion, Hfus = 4.94 kJ/mol

Heat (Q) =..?

Next, we shall determine the number of mole in 100g of ethanol, C2H5OH. This is illustrated below:

Mass of C2H5OH = 100g

Molar mass of C2H5OH = (2x12)+ (5x1) + 16 + 1 = 46g/mol

Number of mole (n) of C2H5OH =..?

Mole = Mass /Molar Mass

Number of mole (n) of C2H5OH = 100/46 = 2.174 moles.

Now, we can obtain the heat required to melt the ethanol as follow:

Q = n x Hfus

Q = 2.174 mol x 4.94 kJ/mol

Q = 10.74KJ

Therefore, 10.74 KJ of heat is required to melt the ethanol.

B. Data obtained from the question include the following:

Mass of C2H5OH = 100g

Heat of vaporisation, Hvap = 38.6 kJ/mol

Heat (Q) =..?

As calculated above, the number of mole in 100g of ethanol, C2H5OH is 2.174 moles.

The heat required to vaporise the ethanol can be obtained as follow:

Q = n x Hvap

Q = 2.174 mol x 38.6 kJ/mol

Q = 83.92 KJ

Therefore, 83.92 KJ of heat is required to vaporise the ethanol.

C. From the above calculations, a higher amount of heat energy i.e 83.92 KJ is required to vaporise the ethanol and a lesser amount of heat energy i.e 10.74 KJ is needed to melt the ethanol.