Section 1
Preview this deck
How do the particles move in a liquid?
Front
| 5 | 0 | ||
| 4 | 0 | ||
| 3 | 0 | ||
| 2 | 0 | ||
| 1 | 0 |
Active users
0
All-time users
0
Favorites
0
Last updated
6 years ago
Date created
Mar 1, 2020
Cards (130)
Section 1
(50 cards)
How do the particles move in a liquid?
The particles in a liquid are free to move.
A Gas has volume of 0.572L at 35.0C and 1.00atm pressure. What is the temperature inside a container where this gas has a volume of 0.535L at 1.00atm?
288K
A pressure is what?
Exerted when the gas particles collide with the walls of any container it is held in.
Since solids and liquids tend to have their particles very close together. Their volumes are often very similar. What does this mean?
They have strong forces of attraction.
If a 1.23L sample of a Gas at 53.0 torr is put under pressure up to a value of 240. Torr at a constant temperature, what is the new volume?
0.272L
Convert 830 torr to atmospheres
1.09 atm
Describe the movement of particles in the solids as crystalline or amorphous.
In both cases, the particles in the solid have very little energy and move very little in relation to one another. They are sometimes described as 'vibrating around fixed positions.'
Describe the shape and volume of a solid.
Definite shape and definite volume.
All the properties of solids and liquids such as viscosity, surface tension, hardness etc., are dependent upon what?
1. How the particles that make up the solid or liquid are arranged 2. The extent of the attractions between those particles
*These assumptions do have limitations. For example, gases can be liquified if cooled enough. This means "real" gas particles do attract one another to some extent; otherwise the particles would never stick to one another and therefore never condense to form a liquid.*
What are the categories that solids broadly fall into?
Crystalline And a amorphous
What is the equation for Avogadro's Law?
V1/n1=V2/n2
What are the distinct characteristics of matter?
It has mass and it occupies space.
What is a real-world example of Boyle's Law?
Squeeze ballon
As a result of the large amount of empty space in a volume of gas, gases are ____________________?
Easily compressed
What are the five postulates of the Kinetic molecular theory?
1. Gases are composed of tiny particles (atoms or molecules) whose size is negligible compared to the average distance between them; the total volume that the gas fills is almost all empty space; the observation that gases are compressible. 2. The gas particles move randomly, in straight lines, in all directions and at various speeds. 3. The forces of attraction or repulsion between two gas particles are negligible, except when they collide. 4. When particles collide with one another, the collisions are elastic. The collisions with the walls of the container create the gas pressure. Elastic collisions do not spontaneously convert to the liquid. 5. The average kinetic energy of a molecule is proportional to the Kelvin temperature and as a result, all calculations involving gases should be carried out with temperatures converted to K.
Describe the shape and volume of a liquid.
Have no shape of their own but take the shape of their container. A liquid has a definite volume.
Convert 657 mmHg to atm
0.864 atm
What is the relationship between Avogadro's Law?
Volume and moles
What does Charles' Law state?
At constant pressure, volume is directly proportional to temperature.
Describe the shape and volume of gases.
Have neither a definite shape nor a definite volume.
How do the particles move in a solid?
The particles in a solid are packed tightly together and only vibrate gently around fixed positions.
For Avogadro's Law, what does a constant equal?
V/n
What is the equation for Charles' Law?
V1/T1=V2/T2
What is the relationships with Boyle's Law?
Pressure and volume
For Charles' Law, if the temperature is increased the gas particles ______________ kinetic energy, ________________?
Gain; move around move and occupy more space
*1.00 atm= 760. mmHg= 760. Torr* ON EQUATION TABLE
Define amorphous.
Where the arrangement of particles is not regular or ordered.
If 2.11g of neon gas occupies a volume of 12.0L at 28.0C. What volume will 6.58g of neon occupy under the same conditions?
37.3L
What are the relationships with Charles' Law?
Volume and temperature
What is the equation for Boyle's Law?
P1V1=P2V2
What is the equation for Gay-Lussac's Law?
P1/T1=P2/T2
The pressure on a 411mL sample of gas is decreased from 812mmHg to 790mmHg. What will the new volume of the gas be?
422mL
Define crystalline.
Where a regular, ordered, repeatable 3-D Structure of particles is found.
*Since, in a Gas, the particles possess enough energy to overcome any intermolecular forces and hence move around completely freely and with large spaces between them, a liquid represents particles in an intermediate state between the extremely ordered and low energy state of a solid, and the extremely disordered and high energy state of a Gas.*
What does Avogadro's Law state?
At constant temperature and pressure, volume is directly proportional to the number of moles of gas present. This means that the volume of a gas increases with increasing number of moles, and vice versa.
A Gas has no definite ___________________ and will expand to ______________?
Shape or volume; fill as much space as possible
For Gay-Lussac's Law, what is the constant?
P/T
How do the particles move in a Gas?
The particles in a Gas spread apart filling all the space of the container available to them.
For Charles' Law, what does the constant equal?
V/T
What is the relationship between Gay-Lussac's Law?
Pressure and temperature
Describe the movement of particles in liquids.
Particles in liquids are constantly moving and colliding with one another, have significantly greater energy and move a lot in relation to one another.
An 11.0L sample of a Gas is collected at 276K and then cooled by 14K. The pressure is held constant at 1.20atm. Calculate the new volume of the gas.
10.4L
A 13.1L sample of 0. 502 moles of 02 is held under conditions of 1.00atm and 25C. If all of the O2 is then converted to ozone (O3) what will be the volume of ozone?
8.74L
Define viscosity.
Thickness- resistance to motion
For Boyle's Law, if the volume is increased, the gas particles ______________?
Collide with the walls of the container less often and the pressure is reduced.
What does Boyle's Law state?
At constant temperature, pressure is inversely proportional to volume. This means that as the pressure increase the volume decreases and vice versa.
Gases are made up of particles that have what kind of energy?
(Relatively) large amounts
Solids fall broadly into how many categories?
Two
What is the basis for many properties of gases?
The Kinetic molecular theory
Section 2
(50 cards)
What does Dalton's Law state?
In a mixture of ideal gases the total pressure exerted by the mixture is equal to the sum of the individual partial pressures of each Gas.
What is the equation for the root mean square speed?
Urms = _/3RT/M
*High pressures and low temperatures experience ________________ and are _________________?*
*Induced dipoles; polarizable (see picture on Dingle Notes)*
What is the equation for Dalton's Law?
Ptotal= P1+P2+P3 etc.
Calculate the number of moles of hydrogen present, in a 0.641L mixture of hydrogen and water vapor, at 21C, that has a total pressure of 750. Torr, given that the vapor pressure of water at this temperature is 20.0 torr.
0.0255mol
HCl vs. NH3— where would the attraction be closer?
HCl: 36 g/mol NH3: 17 g/mol Closer to HCl because NH3 is lighter & travels faster
How much faster is H2 than CO?
3.72 (no units)
A Gas exerts a pressure of 900mmHg at 20C. What temperature would be required to lower the pressure to 1.00atm?
247K
What is the equation for general and combined gas equations?
P1V1/n1T1=P2V2/n2T2
What happens to all random motion?
It ceases.
*The Assumption that the forces of attraction or repulsion between two particles in a Gas are very weak or negligible begins to fail. — Low temperature means less energy, so the particles are attracted to one another more* — What does this mean?
Temporary induced dipoles!
Under these conditions (high P and low T), gases are said to behave non-ideally or like 'real' gases. This has two consequences which are?
1. The real gas situation necessitates the need to correct the volume by subtracting a factor. 2. The observed pressure is less than in an ideal gas.
*REVIEW GRAPHS IN NOTES OF BOYLE'S AND CHARLE'S LAW*
What does Gay-Lussac's Law state?
At constant volume, pressure is directly proportional to temperature. This means that temperature increases with increasing pressure, and vice versa.
What is the universal gas constant (R)?
0.0821 L atm K^-1 mol^-1
For Henry's Law, if the answer is greater than one ________________?
Then the first in the problem is lighter, faster than the second element/compound in the problem.
Effusion is _________________?
The process in which a gas escapes from one vessel to another by passing through a very small opening.
For the ideal gas law, describe the particles.
They do not attract one another (they act independently)
What does n equal in the PV=nRT equation?
mass/molar mass= g/g/mol= mol
What can be said about the Urms of a gas in relation to its molar mass and in relation to its temperature?
The higher the molar mass, the Urms should be lower because it is heavier. The higher the temperature, the more kinetic energy.
For Henry's Law, Gas solubility usually ________________ with increase of temperature of the solution.
Decreases
How proportional is Boyle's Law?
Inversely proportional between volume and pressure
The root-mean-square-speed of the velocities of gas particles is _______________?
The square root of the averages of the square of the speeds of all the particles a sample at a particular temperature
For Henry's Law, if the answer is equal than one ______________?
Then the elements/compounds in both of the problem share the same speed and mass.
*When the gas is pressurized into a small space that gas particles size becomes _________________?*
More significant compared to the total volume.
What must the molar mass be for the root mean square speed?
In kilograms
At ______________________ gas particles come close enough to one another to make the two postulates of the Kinetic molecular theory invalid.
High pressures and low temperatures
N2 vs. O2— Where would the attraction be closer?
N2: 28g O2: 32g Closer to O2 because N2 is lighter and travels faster.
Henry's Law example: low temperature equals ____________?
More carbonate.
A Gas at 25C In a closed container has its pressure raised from 150. atm To 160. atm. What is the final temperature of the gas?
318K
Engineers/scientists can't use PV=nRT at high pressure to predict __________________? Answers would be __________________?
Properties of gases; incorrect
A sample of aluminum chloride weighing 0.100g was vaporized at 350.C and 1.00atm pressure to produce 19.2mL of vapor. Calculate a value for the molar mass of aluminum chloride.
267g/mol
Henry's Law example: Coke bottles under ____________ pressure, ___________ carbonation CO2 (g)
High; more
What is the equation for the ideal gas law?
PV=nRT
What happens when all random motion ceases?
It cannot be attained.
*What is the equation you must have memorized for pressure?*
P=densityRT/molar mass
What is the assumption that gases are composed of tiny particles?
Whose size is negligible.
In Van Der Waals equation, what does the a stand for?
Relatively strong inter particle attractions for one another would have corresponding relatively large values (intermolecular forces)
For Henry's Law, what is the direct proportion?
Pressure and solubility.
How proportional is Charles' Law?
Directly proportional between temperature and volume
Assuming ideal behavior, how many moles of helium gas are in a sample that has a volume of 8.12L at a temperature of 0.00C and a pressure of 1.20 atm?
0.435mol
In Van Der Waals equation, what does the b stand for?
Relatively large gas particles would have correspondingly relatively large values since they take up a larger volume (volume)
3.00L of Carbon monoxide gas at a pressure of 199. kPa, And 1.00L of carbon dioxide gas at a pressure of 300. kPa are injected into a 1.25L container. Assuming no reaction between the two gases, what is the total pressure in this container?
717.6kPa
Diffusion is ________________?
The process by which a homogenous mixture is formed by the random mixing of two different gases.
For Henry's Law, if the answer is less than one ______________?
Then the first in the problem is heavier, slower than the second element/compound in the problem.
If the number of moles of a Gas in an experiment is constant (frequently the case), what is the equation?
P1V1/T1=P2V2/T2
What must the R be in the root mean square speed equation?
8.314kgm^2/s^2molK
Rate of effusion A/Rate of effusion B equals what?
_/density of B/density of A OR _/Molar mass of B/Molar mass of A
For Henry's Law, at higher pressures more gas particles strike the surface of the solution and enter the solution, meaning ___________________?
The concentration of the gas dissolved in the solvent is greater.
The combination of Laws above leads to the formulation of the ________________?
Ideal gas law
Section 3
(30 cards)