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Describe the motion of the particles in solids
Particles cannot move, they can only vibrate in fixed positions
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Key Terms
Term
Definition
Describe the motion of the particles in solids
Particles cannot move, they can only vibrate in fixed positions
Describe the motion of the particles in liquids
Particles have more energy and can break away and slide over each other
Describe the motion of the particles in Gas
Particles have the most energy and are widely spaced moving at great speed
What is diffusion?
Diffusion is the movement of a substance from an area of high concentration to an area of low concentration
What are the factors involved when describing gases?
Temperature, Pressure - the force a gas exerts on a unit area, Volume
How do you turn degrees into kelvin?
+273
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| Term | Definition |
|---|---|
Describe the motion of the particles in solids | Particles cannot move, they can only vibrate in fixed positions |
Describe the motion of the particles in liquids | Particles have more energy and can break away and slide over each other |
Describe the motion of the particles in Gas | Particles have the most energy and are widely spaced moving at great speed |
What is diffusion? | Diffusion is the movement of a substance from an area of high concentration to an area of low concentration |
What are the factors involved when describing gases? | Temperature, Pressure - the force a gas exerts on a unit area, Volume |
How do you turn degrees into kelvin? | +273 |
How do you turn pascals into kilopascals? | Divide by 1000 |
What is Boyle’s law? | Boyle's law states that for a definite mass of gas at a constant temperature, pressure is inversely proportional to volume (P1V1 = P2V2) |
What is Charles law? | Charles law states that for a definite mass of a gas at constant pressure, volume is directly proportional to temperature (ONLY WHEN IN KELVIN) V1/T1 = V2/T2 |
What is the combined gas law? | P1V1/T1 = P2V2/T2 conditions 1 = conditions 2 |
What is Gay- Lussac’s law of combining volumes? | In a reaction between gases there is a simple whole number ratio of volumes of reactants and products at the same conditions of temperature and pressure |
What is Avogadro’s law? | It states that equal volumes of gases at the same conditions of temperature and pressure have equal numbers of molecules (and therefore equal number of moles) |
Volume of any gas at standard temperature and pressure (s.t.p) | 22.4L |
Volume of any gas at room temperature and pressure | 24 L |
Outline the assumptions of the kinetic theory of gases | Gases are made up of particles in continuous, rapid, random, straight line motion, colliding with each other and within the walls of their container. There are no attractive or repulsive forces between the molecules of a gas. The volume of the molecules is negligible compared to the space they occupy. Collisions between molecules are perfectly elastic - no loss of kinetic energy. The average kinetic energy of molecules is directly proportional to the temperature in kelvin. |
What is an ideal gas? | An ideal gas is one that perfectly obeys all the gas laws under all conditions of temperature and pressure |
Outline why real gases deviate from ideal gas behaviour/What are limitations of the kinetic theory of gases? | Real gases have attractive forces between their molecules- intermolecular forces. The volume of molecules is not always negligible compared to the space they occupy |
At what conditions do real gases come closest to ideal gas behaviour? | At low pressures - molecules are widely spaced. At high temperatures - molecules have enough energy to overcome attractive or repulsive forces |
Which of the noble gases would you expect to behave most like an ideal gas? Justify your answer | Helium. Ideal gases have no attractive or repulsive forces between the molecules. Helium is the noble gas with the smallest mass and therefore has the weakest (van der Waals) forces |
What is the Ideal gas equation? | pV=nRT pressure (Pa) Volume (m3) number of moles of gas universal gas constant =8.3 temperature (K) |
Describe the procedure of measuring the relative molecular mass of a volatile liquid (using a conical flask) | Use electronic balance, get mass of clean conical flask, rubber band and aluminum foil. Add small volume of propanone/cyclohexane place in beaker full of water, prick foil with hole, fasten with rubber band. Heat water with hotplate close to boiling point, vaporizing the propanone. Allow conical flask to cool to room temp, vapor will condense. Dry outside and find mass. Subtract initial mass from final, this gives the mass of the volatile liquid that has vaporized and condensed again. Calculate the relative molecular mass of a volatile liquid. |
What is meant by a volatile liquid? Name a volatile liquid suitable for this experiment | A liquid with a low boiling point. Propanone/cyclohexane |
How is the temperature of the vapor obtained? | Using a thermometer to measure the temperature of the water- the temperature of the vapor can be assumed to be equal to the temperature of the water |
How is the pressure of the vapor in the conical flask measured? | A barometer is used to measure atmospheric pressure. The pressure of the vapor in the conical flask will be the same as atmospheric pressure due to the pin hole made in the foil |
How is the volume of the volatile liquid found? | The volume of the vapor is found by filling the conical flask that will be filled with the vapor completely with water, pouring it in a graduated cylinder and reading its volume |
Why is this method unsuitable for non-volatile liquids? | The boiling points of non-volatile liquids are too high, boiling water will not vaporize them. |
What modern instrumental technique can be used as a more accurate method to measure the relative molecular mass of volatile and non-volatile liquids as well as of solid and gaseous substances? | Mass spectrometry |
Give three errors in this experiment that may lead to inaccurate results | The entire conical flask should be covered in boiling water to ensure the temperature of the vapor is the same temperature of the water- which is difficult to achieve. The outside of the conical flask and aluminum foil may not be completely dry when finding out their mass for the second time. The electronic balance may only read to an accuracy of one or two decimal places. |