Question

#1
How does kinetic molecular theory explain Dalton's law?

Select the correct answer below:

Question options:

Gas particles collide with the container with the same frequency regardless of whether other gases are present.

Gas particles are different sizes and do not contribute equally to the overall pressure, based on size.

Gas particles contribute to the overall pressure based on their molar masses.

Gas particles have inelastic collisions, based on their individual identity.

Question #2
How does kinetic molecular theory explain gas pressure inside a balloon?

Select the correct answer below:

Question #2 options:

Gas particles are large and only a few fit inside a balloon, inflating the walls.

The atmospheric pressure is greater than the pressure of the gas inside the balloon, so the balloon expands

Gas particles are very small, and many will fill the inside of the balloon until they are all stationary and touching each other.

The pressure exerted by a gas in the balloon results from collisions between the gas molecules and the balloon walls.

Question #3
Why do gases deviate from ideal behavior at high pressure?
Select the correct answer below:

Question #3 options:

The particle volume becomes significant.

The particles have no attraction for one another.

The particle collisions become elastic.

The particles stop moving completely.

Question #4
Which correction term is most important at high pressures?

(P + n2aV2)x (V?nb)=nRT
Select the correct answer below:

Question #4 options:

a

b

R

T

Answer 1

Ans 1

Dalton's law states that in a mixture of non reacting gases, total pressure is equal to the sum of partial pressure of each species inside the mixture.

Every gas contributes to the total pressure but not equally.

It depends on the size of the gas particles.

Gas particles are different sizes and do not contribute equally to the overall pressure, based on size.

Option B is the correct answer

Option A is incorrect because the frequency is not same

Option C is incorrect because it's based on the size of the particles

Option D is incorrect because gas particles have elastic collision.