Topic 5 - Kinetic Theory and Gases Flashcards
How are the particles arranged in a solid?
- Strong forces of attraction hold particles together in fixed, regular arrangement
- Particles don’t have much energy so can only vibrate about their fixed positions
How are the particles arranged in a liquid?
- Weaker forces of attraction between particles
- Particles are close together but can move past each other + form irregular arrangements
- Have more energy than particles in solids so move in random directions at low speeds
How are the particles arranged in a gas?
- Almost no forces of attraction between particles
- Particles have more energy than those in liquids/solids
- Free to move + travel in random directions at high speeds
- Consist of very small particles (kinetic theory)
- Particles constantly moving + colliding w/ each other + walls of container
- When they collide, bounce off each other or walls
- Hardly take up any space, most of the gas is empty space
What are the three states of matter?
- Solid
- Liquid
- Gas
What is absolute zero?
- Increase temp = higher KE, decrease temp = lower KE
- Coldest possible temp
- As little kinetic energy as possible to get
- 0K
How do you convert from kelvin to °C?
-273
How do you convert from °C to kelvin?
+273
For every 1°C increase, how many kelvins does it increase by?
1
What is absolute zero in °C and kelvin?
- -273°C
- 0K
What is the freezing point of water in °C and kelvin?
- 0°C
- 273K
What is the boiling point of water in °C and kelvin?
- 100°C
- 373K
What is the relationship between kinetic energy and temperature?
- Kelvin temperature of a gas is directly proportional to average kinetic energy of its particles
- If increase temp, particles have more energy, double temp = double average KE
What does the kinetic theory say about colliding gas particles?
- As gas particles move they collide w/ each other/anything else in their way
- Gas particles are very light but not massless so when collide exert force on it
- In sealed container gas particles hit container walls creating outward pressure
- Pressure depends on how fast particles are moving + how often hit walls
What is the relationship between volume and temperature of a gas when pressure is constantly?
Proportional (heat up particles have more energy so move faster expanding + taking yo more room, so volume increases)
What is the equation linking volume and temperature when pressure is constant?
Volume1 = (volume2 x temperature p1) / temperature2
Temperature must be in K
V1=(V2xT1)/T2
V1 + T1 are starting conditions + V2 + T2 and final conditions
V/T=constant
What is the relationship between pressure and volume at a constant temperature?
- Inversely proportional
- As pressure increases, volume decreases + vice versa
- Bigger container has fewer collisions between gas particles + container walls o
What is the equation to show the relationship between pressure and volume at a constant temperature?
V1 x P1 = V2 x P2
Fixed mass
V1 + P1 = initial volume + pressure, V2 + P2 = final volume + pressure
How can you use a gas syringe to investigate volume and temperature at a constant pressure?
- Half full gas syringe w/ air + seal w/ rubber bung
- Use Bunsen burner to heat air in gas syringe
- As it heats, gas expands, pushing plunger outwards, volume of gas increases as temp increases
- Since syringe plunger free to move pressure of gas always same
- If cooled again gas will contract pulling plunger in
