Standard 4: Gases. Chemistry. Ms. Siddall. Standard 4f: Lowest Possible Temperature Absolute zero = temperature where there is no particle movement (no kinetic energy). There can be no lower temperature. absolute zero = 0 Kelvin = 0K Deep space ~ 2.7K Summary 1 At what temperature do particles stop moving? Standard 4e: Kelvin/Celsius conversions Kelvin temperature = °C + 273 Example: room temperature is about 22°C. What is that in Kelvin? Kelvin = °C + 273 = 22 + 273 = 295K Example: What is 0K in °C? °C = Kelvin - 273 = 0 - 273 = -273°C Summary 2 1. Convert 100°C to Kelvin 2. Convert 100K to Celsius Standard 4d: Standard Temperature and Pressure STP: 1 mole of gas = 22.4L Temperature = 0°C = 273K Pressure = 1 atm Summary 3 One mole of gas at 0°C has a volume of 22.4L. What is the pressure of the gas? 4a: Pressure Atmospheric pressure = force of air hitting you Particles are in constant motion Particles have mass Mass x motion = force Force = pressure Summary 4 What causes atmospheric pressure? Measuring pressure Atmospheric pressure = 1atm (atmosphere) 1atm = 760 Torr = 760mmHg = 29.9inHg = 101,325 Pa = 101.325kPa = 14.7psi (lb/in2) Example: Coca-Cola© is bottled at approximately 2 atmospheres. Convert to Torr. 2 atm 760 Torr 1 atm ~ 1520 Torr Summary 5 Convert 2atm to: 1. Psi 2. kpa Liquids and gases compared • Atmospheric pressure = 14.7psi • Deep ocean pressure = 16,000psi • Water molecules are close together (high pressure) and air particles are far apart (lower pressure) • Density of water = 1g/ml = 1000g/L • Density of air = 1g/L Summary 6 Explain the difference between molecules in a liquid and molecules in a gas. Kinetic Molecular Theory: 1. Gases consist of small particles that have mass. 2. The volume of a gas is mostly empty space. 3. There are no intermolecular attractions between gas particles. 4. Particles are in constant, random, rapid, straight line motion. 5. Collisions are elastic (no loss of energy). 6. Kinetic energy of particles depends on temperature. Summary 7 Which two points of the Kinetic Molecular Theory explain pressure? (remember pressure = mass x motion) Temperature measures average kinetic energy. Individual particles have different energies. Most molecules have average kinetic energy Summary 8 According to the graph: Which temperature shows the highest average kinetic energy? Summary 9 Which points of the Kinetic Molecular Theory explain these properties? Gases are compressed easily Gases fill their containers 4b: Diffusion Diffusion = ability of gases to mix Particles move constantly Particles are not attracted to each other Therefore: Particles fill a container Particles form a homogeneous mixture Lighter gases diffuse more quickly Heavy gases diffuse more slowly Summary 10 What is a homogeneous mixture? Summary 11 Helium gas and oxygen gas are released into a room at the same time. Which gas fills the room first? Explain why. Dalton’s Law The total pressure of a mixture of gases is the sum of the pressure of each gas: Ptotal = P1 + P2 + P3 + …. Summary 12 At the summit of mount Everest the total pressure is about 0.3atm. Assume PTotal = PN2 + PO2 If PN2 = 0.25atm what is the pressure of oxygen? 4c: The Gas Laws The combined gas law: for changing conditions P1V1 = P2V2 T1 T2 Initial conditions P1 V1 Initial pressure (atm) T1 Initial temperature* (K) Initial volume (L) Final conditions P2 V2 Final pressure (atm) T2 Final temperature* (K) Final volume (L) *Temperatures must be in Kelvin only Example: a gas at STP has a volume of 10L. The pressure is increased to 5atm. Temperature remains constant. What is the new volume? Initial conditions P1 1 atm Final conditions P2 5 atm V1 10L V2 ? T1 273K T2 = T1 P1V1 = P2V2 T1 T2 P1V1T2 = P2V2T2 T1P2 T2P2 Example: A plane flies at 35,000 feet. Pressure outside is 0.25atm. Temperature in the cabin is 27°C. What will the temperature be if the cabin loses pressure? Initial conditions Final conditions P1 1 atm P2 0.25 atm V1 =V2 V2 =V1 T1 300K T2 ? P1V1 = P2V2 T1 T2 T1 = T2 P1V1 P2V2 Summary 13 A gas has a fixed volume and a pressure of 1atm. If temperature increases from 200K to 400K what is the new pressure? Relationships using the Gas Law. Pressure vs. Volume VP VP Pressure (atm) = inverse relationship = inversely proportional Smaller volume = more collisions = more pressure volume (L) Summary 14 If the volume is decreased by a factor of 3, what happens to the pressure? Temperature vs. pressure pressure (atm) T P T P = direct relationship = directly proportional Higher temperature = more energy = more collisions = more pressure Temperature (K) Summary 15 If the temperature is tripled, what happens to the pressure? Volume vs. Temperature Volume (L) T V T V = direct relationship = directly proportional Temperature (K) Higher temperature = more energy Gas takes up more space Summary 16 If the temperature is decreased by a factor of 4 what happens to the volume of the gas? moles vs. pressure n (=number of moles) P n P = direct relationship = directly proportional More gas = more collisions = more pressure Summary 17 If the number of particles is doubled, what happens to the pressure? Honors Only 4h: solve problems by using the ideal gas law in the form PV = nRT Ideal Gas Law PV = nRT P = pressure (atm) V = volume (L) n = number of moles R = universal gas constant = 0.0821L·atm/mol·K T = temperature (K) Example: what is the volume of 1 mole of gas at standard temperature and pressure? PV = nRT V = nRT/P V = (1 mol)(0.0821L·atm) (273.15K) (mol·K) (1 atm) V = 22.4L Summary 18 At 500°C what is the pressure of one mole of gas that has a volume of 10L? The Ideal Gas Law (and the Combined Gas Law) only work under ‘ideal conditions’ Ideal conditions = moderate temperature & pressure Non-ideal conditions: (when the gas laws no longer makes good predictions) Extremely high pressure: Particles are too close together Particles take up space Extremely low temperature: Particles have very low energy Particles are attracted to each other Summary 19 Explain why the inverse relationship between pressure and volume is not linear 4i:apply Dalton’s Law of Partial Pressures to describe the composition of gases and Graham’s Law to predict diffusion of gases Graham’s Law: rate = (1/mass) The rate of diffusion depends on particle mass Gases with lower mass diffuse faster Effusion: rate of gas passing through a small opening in a container Summary 20 Which gas will effuse faster; chlorine or bromine? Why? 4g: the kinetic molecular theory relates the absolute temperature of a gas to the average kinetic energy of its molecules or atoms At 0K all motion ceases At 0K: average kinetic energy = zero Summary 21 If the average kinetic energy of a gas is zero, what is the temperature of that gas in Kelvin? Why?