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3 years ago

How is the kinetic energy of the particles that make up a substance different

Chemistry

1 answer:

erastova [34]3 years ago

8 0

Answer:

D. The kinetic energy is greater after a substance changes from a

solid to a liquid

Explanation:

During a phase change from solid to liquid, the particles making up the mobile becomes more mobile and as a result there is an increase in kinetic energy of the system.

Kinetic energy is the energy accrued due to the motion of a body.
In a melting process where solids turn to liquid, there is an increase in kinetic energy.
When randomness of a system increase, kinetic energy also increases.
From liquid to gas and gas to plasma increases kinetic energy.
In the other way round, the kinetic energy reduces.

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Ahat [919]

B) As water temp increases solubility increases

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3 years ago

What is the formula for aluminum iodide?

lesya [120]

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3 years ago

What is the atomic mass of aluminum?

love history [14]

Answer:

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Explanation:

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3 years ago

Hydrogen and oxygen react under a specific set of conditions to produce water according to the equation:

Nata [24]

Answer:

1. The amount required of H₂ = 11.0 g.

2. The amount required of O₂ = 88.0 g.

Explanation:

The balanced equation for the mentioned reaction is:

2H₂(g) + O₂(g) → 2H₂O,

It is clear that 2.0 moles of H₂ react with 1.0 mole of O₂ to produce 2.0 moles of H₂O.

Q1: How much hydrogen would be required to produce 5.5 mol of water?

Using cross multiplication:

2.0 mol of H₂ produce → 2.0 mol of H₂O, from stichiometry.

??? mol of H₂ produce → 5.5 mol of H₂O.

∴ the no. of moles of H₂ needed to produce 5.5 mol of water = (2.0 mol)(5.5 mol)/(2.0 mol) = 5.5 mol.

Now, we can get the mass of H₂ needed to to produce 5.5 mol of water:

mass of H₂ = (no. of moles)(molar mass) = (5.5 mol)(2.0 g/mol) = 11.0 g.

Q2: How much oxygen would be required?

Using cross multiplication:

1.0 mol of O₂ produce → 2.0 mol of H₂O, from stichiometry.

??? mol of O₂ produce → 5.5 mol of H₂O.

∴ the no. of moles of O₂ needed to produce 5.5 mol of water = (1.0 mol)(5.5 mol)/(2.0 mol) = 2.75 mol.

Now, we can get the mass of O₂ needed to to produce 5.5 mol of water:

mass of O₂ = (no. of moles)(molar mass) = (2.75 mol)(32.0 g/mol) = 88.0 g.

5 0

3 years ago

How does a fire extinguisher works ?

Usimov [2.4K]

Answer:

Most fire extinguishers work by separating the fuel from the oxygen. The oxygen comes from the air. It is the same oxygen we breathe. Since the oxygen has to be in contact with the fuel, if you can coat the fuel with something that keeps the oxygen away, the fire will go out. Some ways of using fire extinguisher are:

 Water extinguishers work mainly by cooling (removing heat), but a dense spray of water droplets also helps to cut off oxygen.

 Dry powder extinguishers soak up heat, melt on the fuel, and cut off oxygen, but they also neutralize the fuel (cutting it off from the fire) .

Explanation:

I hope it was helpful...

8 0

1 year ago