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tia_tia [17]
3 years ago
14

In which state do molecules have the highest kinetic energy? in the liquid state in the solid state in the gaseous state during

the phase change from liquid to gas
Chemistry
2 answers:
Ipatiy [6.2K]3 years ago
8 0

Answer: Option (c) is the correct answer.

Explanation:

Kinetic energy is defined as the energy obtained by an object or substance due to their motion.

Also, kinetic energy is directly related to temperature as follows.

                        K. E = \frac{3}{2}kT

Hence, kinetic energy is directly proportional to temperature.

So, more is the temperature provided to a substance more will be the kinetic energy of its molecules. Therefore, more will be their motion and this leads to more number of collisions between the molecules.

As in solids, molecules are held by strong intermoleculear forces so, they do not move from their initial position and hence, they have definite shape and volume.

In liquids, molecules are held by less strong intermolecular forces of attraction. So, they have definite volume but no definite shape.

In gases, molecules are held by weak intermolecular forces. So, these molecules are away from each other due to high kinetic energy as they have more number of collisions.

Thus, we can conclude that in the gaseous state molecules have the highest kinetic energy.

Dvinal [7]3 years ago
5 0
It depends on the substance,but for most substance it is in the gaseous state.
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How does the appearance of a substance change when it<br> changes phase?
kicyunya [14]

Answer:

Melting: the substance changes back from the solid to the liquid. Condensation: the substance changes from a gas to a liquid. Vaporization: the substance changes from a liquid to a gas. Sublimation: the substance changes directly from a solid to a gas without going through the liquid phase.

Explanation:

6 0
3 years ago
ICl has a higher boiling point than Br2. What is the best explanation for this?
Flura [38]
<span>The best answer is B. ICl experiences induced dipole-induced dipole interactions. Both iodine and chlorine belongs to the same group of the periodic table. Electronegativity decreases as you go down a group therefore Cl will have a greater attraction with the bond it forms with another atom. Dipole-dipole interactions form between I and Cl. For the Br2 molecule, no dipole occurs because they are two identical atoms. Therefore we will be expecting ICl will have a higher boiling point due to higher binding energy it forms.</span>
7 0
3 years ago
PLEASE PLEASE HELP ME!!!A 450 ml gas sample has a pressure of 1.25 atm at 65 °C. What is the temperature, in °C, at which the ga
Arlecino [84]

Answer:

89°C

Explanation:

Combined Gas Law (P₁V₁)/T₁ = (P₂V₂)/T₂

(1.25 atm)(450 mL)/(65°C) = (0.89 atm)(865 mL)/T₂

8.653846154 = 769.85/T₂

T₂ = 769.85/8.653846154

T₂ = 88.96044444 = 89°C

6 0
3 years ago
A chemist combined 0.440 L of an unknown calcium solution with an excess of ammonium chromate. This resulted in the precipitatio
Rina8888 [55]

The concentration of the original calcium ions is 0.005 M

<h3>What is concentration?</h3>

The term concentration has to do with the amount of substance in solution. We know that the concentration can be measured in a lot of units such as mole/litre, grams per litre, percentage and so on.

As such we have the equation;

Ca^2+(aq) + (NH4)2CrO4(aq) --------> CaCrO4(s) + 2NH4^+(aq)

Number of moles of the precipitate = 346.7 * 10^-3 g/156 g/mol

= 0.0022 moles

Now;

1 mole of Ca^2+ produces 1 mole of CaCrO4 hence 0.0022 moles of CaCrO4 was produced by  0.0022 moles of CaCrO4.

Given that the volume of the solution is  0.440 L, the concentration of the solution is;   0.0022 moles/0.440 L

= 0.005 M

Learn more about molarity:brainly.com/question/8732513

#SPJ1

6 0
1 year ago
4. Calculate the final concentration if water is added to 1.5 L of a 12 M
konstantin123 [22]

Answer:

6M

Explanation:

(Molarity x Volume)concentrated soln = (Molarity x Volume)diluted doln

Molarity dilute soln = [(M x V)conc/V (dilute)] = 1.5L x 12M / 3.0L = 6M final dilute soln

6 0
3 years ago
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