Gases

Question 1

Boyle’s law

Answer 1

Volume and PRESSURE is an Inverse relationship

Question 2

Charles’s Law

Answer 2

Volume and TEMPERATURE have a direct relationship

Question 3

Avogado’s law

Answer 3

Volume and MOLES have a direct relationship

Question 4

Dalton’s gas law

Answer 4

the total pressure exerted is equal to the sum of the partial pressures of the individual gases

Question 5

Celsius to Kelvin

Answer 5

+273(.15)

Question 6

KPa to ATM

Answer 6

101.3 KPa - 1 atm

Question 7

mmHg to atm

Answer 7

760 mmHg - 1 atm

Question 8

torr to atm

Answer 8

760 torr - 1 atm

Question 9

psi to atm

Answer 9

14.7 psi - 1atm

Question 10

Ideal Gas Law

Answer 10

pv=nRt or PV/NT = R

Question 11

STP

Answer 11

1 ATM, 273K, 22.4 L, 1 Mole

Question 12

Absolute 0 temp

Answer 12

0 Celsius or -273 Kelvin

Question 13

water vapor

Answer 13

subtracted when using a barometer, affected by temp

Question 14

Postulates of the Kinetic Molecular Theory of Gases (5)

Answer 14

Gases consist of tiny particles (atoms or molecules).

These particles are so small, compared with the distances between them, that the volume (size) of the individual particles can be assumed to be negligible (zero).

The particles are in constant random motion, colliding with the walls of the container. These collisions with the walls cause the pressure exerted by the gas.

The particles are assumed not to attract or to repel each other.

The average kinetic energy of the gas particles is directly proportional to the Kelvin temperature of the gas.

Question 15

Kinetic energy formula

Answer 15

𝐾𝐸=1/2𝑚𝑣^2 (m-mass v-velocity)