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2 years ago

PLEASE HELP

Chemistry

1 answer:

charle [14.2K]2 years ago

8 0

Answer: The statement, average kinetic energy of the gas particles is greater in container A because its particles move faster is correct.

Explanation:

Kinetic energy is the energy obtained due to the motion of an object or substance.

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

where,

T = temperature

This means that kinetic energy is directly proportional to temperature.

So, when heat is provided to container A then its molecules will start to move rapidly from one place to another which will cause more collisions between the atoms.

Hence, average kinetic energy will be more in container A.

Whereas container B is placed at room temperature which is low than that in container A. So, molecules in container B will move at almost same speed and therefore, specific collisions will be there. So, average kinetic energy in container B will be less than that in container A.

Thus, we can conclude that the statement, average kinetic energy of the gas particles is greater in container A because its particles move faster is correct.

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___________________________________________________________

BONUS METHOD TIME!!!

We know the relation:

M1 * V1 = M2 * V2

where M1 and M2 are the initial and final molarities and V1 and V2 are initial and final volumes respectively

notice that I didn't mention that the volume has to be in Liters, that's because of the units being concerned with both sides of the equation, say I have the volume in mL and want to convert both these volumes to L, I would divide both sides by 1000, which would NOT change the overall value

Now, plugging values in this equation

(0.45) * (251) = (251 + 455)* (M2)

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