The Gas Laws

Question 0

Liquid

Answer 0

Br2

Question 1

Gases Moles to Grams

Answer 1

H2 N2 O2 Fl2 Cl2 up

Question 2

Solid

Answer 2

I2

Question 3

Ionic Compounds

Answer 3

Solid

Question 4

Covalent gases

Answer 4

CO CO2 SO4 SO3 PO3

Question 5

Increase temperature

Answer 5

Increase Energy

Question 6

Lower Temperature

Answer 6

Decrease Energy

Question 7

What happens when Volume Increases?

Answer 7

Pressure Decreases

Question 8

What does P 1 atm equal?

Answer 8

760 mmHg

Question 9

What is volume in ?

Answer 9

L or ML 1L = 1x10 Negative 3

Question 10

How do you convert T into K?

Answer 10

T= Degrees C+273 in K

Question 11

PV/T n=?

Answer 11

P1 V1/ T1 = P2 V2/T2

n= constant not changing

Question 12

V Increases P Decreases

Answer 12

P1 V1 are inversely proportional

Question 13

Charles Law

Answer 13

V1/T1 (K) = V2/T2 (K)

Question 14

Combination gas law

Answer 14

P1 V1/ T1 (K) = P2 V2/ T2 (K)

Question 15

Boyle’s Law

Answer 15

P1 V1 = P2 V2

V,T directly proportional

Question 16

PV=?

Answer 16

nRT

Question 17

n=?

Answer 17

mole

Question 18

One condition quantity

Answer 18

(Kg, g, left or right mole)

Question 19

R=?

Answer 19

Ideal gas constant

Question 20

atm/v

Answer 20

l/v ( change to the proper units before solving x)

Question 21

Ionic Forces

Answer 21

Ionic Compounds

Question 22

Covalent Compounds

Answer 22

London Forces
dipole-dipole interaction
H-bonds (FON)

Question 23

Hydrogen bonds are ?

Answer 23

The strongest dipole dipole (polar)

Question 24

R=PV/nT=?

Answer 24

0.0821 atmxL/molexK

Question 25

Dalton’s law of partial pressure

Answer 25

States that the total pressure exerted by a mixture of gases is the sum of the partial pressures of the individual gases.

Question 26

Partial Pressure

Answer 26

Is the pressure that a gas in a mixture would exert if it were present alone under the same conditions.