Question

Gas Laws Worksheet Name: ah Date: 1224/1g Gas constant R-0.0821 L-atm/K-mol torr I. I atm = mmHg = 2. What is Boyle's law? 3. What is Charles's law? 4. What is ideal gas law? 5. What is STP? 6. Write the assumptions made by the Kinetic Molecular Theory.

Answer 1

1]

1 atm = 760 mm Hg = 760 torr

2]

Boyles law :

For a fixed amount of gas hed at constant temperature , the volume and pressure are inversely proportional to each

other

V proportional to 1/P

PV = constant

3]

Charles law :

For a fixed amount of gas held at constant pressure , the volume is directly proportional to the kelvin temperaure

V is proportional to T

V/T = constant

4]

PV = nRT

A physical law describing the relationship of the measurable properties of an ideal gas, where P (pressure in atm) , V (volume in L) , n (number of moles) , R (the gas constant) , T (temperature in Kelvin). It is derived from a combination of the gas laws of Boyle, Charles, and Avogadro. Also called universal gas law .

5]

STP --> standard temperatuer and pressure

Nominal conditions in the atmosphere at sea level

T = 0C or 273 K and P = 1 atm at STP

6]

Assumptions of Kinetic molecular theory :

1. Gases are composed of a large number of particles that behave like hard, spherical objects in a state of constant, random motion.
2. These particles move in a straight line until they collide with another particle or the walls of the container.
3. These particles are much smaller than the distance between particles. Most of the volume of a gas is therefore empty space.
4. There is no force of attraction between gas particles or between the particles and the walls of the container.
5. Collisions between gas particles or collisions with the walls of the container are perfectly elastic. None of the energy of a gas particle is lost when it collides with another particle or with the walls of the container.
6. The average kinetic energy of a collection of gas particles depends on the temperature of the gas and nothing else.