Gases

Question 1

Liquids and solids are imcompressible

Answer 1

true

Question 2

What are the ideal gas assumptions?

Answer 2

-THe gas particles take up no space/volume themselves -Molecules dont experience any attractive/repulsive/intemolecular forces

Question 3

Under the kinetic molecular theory, the pressure of a sample of gas comes from collisions between gas particles and ______.

Answer 3

the walls of the container

Question 4

True or False: According to kinetic molecular theory, the higher the temperature, the lower the kinetic energy

Answer 4

Fasle, the higher the temp the high the KE

Question 5

True or False: Gases behave least ideally at high pressure and low temperature.

Answer 5

True

Question 6

Which law:

Answer 6

Boyles law, pressure and volume are inversely related.

Question 7

Which law: volume and tempurature of gases are directly related

Answer 7

Charles law

Question 8

Which Law:

Answer 8

Charles

Question 9

Avogadros Law

Answer 9

Volume of gas is directly related to the number of moles of has particle

Question 10

Which Law:

Answer 10

Avogadro

Question 11

At 273 K and 1 Atm, a mole will take up how much space?

Answer 11

22.4 L

Question 12

What is STP?

Answer 12

Standard tempurature and pressure = 1 atm and 0 celcius/273 K . THIS IS NOT THE SAME AS STANDARD THERMODYNAMIC CONDITIONS WHICH IS 1 ATM and 25 CELCIUS (298K)

Question 13

Accoding to boyles law, what would quadrupling the volume of gas do to pressure?

Answer 13

quadrupling the volume of a gas should reduce pressure to one-fourth of what it was before

Question 14

Ideal gas law

Answer 14

PV=nRT

Question 15

Van der waals equation

Answer 15

a accounts for the attraction of the molecules, b counts for the size

Question 16

Mole Fraction of a gas

Answer 16

X=n_gas/n^_total

Question 17

How can you calculate the pressure a single gas exerts in a mixture give the toal pressure and mole fraction?

Answer 17

Pgas= (mole fraction)*(Ptotal)

Question 18

True or false: If Gas A diffused 5 times faster than Gas B, then Gas B must have 25 times the molar mass.

Answer 18

This statement is true. Graham’s law can be used to compare the rates of diffusion of two gases. This equation can be written as rate 1 / rate 2 = √molar mass 2 / √molar mass 1; in other words, the rate of diffusion of a gas varies with the reciprocal of the square root of its molar mass. So, if Gas A diffused 5 times faster than Gas B, then the molar mass of Gas B must be 5^2 = 25 times greater.

Question 19

Henry’s Law

Answer 19

Henry’s law states that the concentration of a dissolved gas equals the partial pressure of the gas multiplied by its molar solubility.

C= k P

where C is the conentration, k is the mols/atm or molarity, and P is the partial pressure of the gas