Chem Ch 5 6 7 8
Fluid Dynamics Quiz
Test your knowledge on fluid mechanics with our comprehensive quiz covering chapters 5 to 8. Dive into the fascinating world of fluids, buoyancy, and gas laws with 81 challenging questions designed for students, teachers, and anyone interested in the principles of physics.
Challenge yourself with topics including:
- Hydrostatics
- Buoyancy and Viscosity
- Bernoulli's Principle
- Kinetic Molecular Theory
- Gas Laws
Match the definitions: | |
|---|---|
Buoyancy | |
Fluid | |
Hydrometer | |
Hydrostatics | |
Laminar flow | |
Turbulent flow | |
Bernoulli's principle | |
Flow rate | |
Archimede's principle | |
Pascal's principle | |
Viscosity |
In what area of a tube will fluid be moving the fastest?
On the sides of the tube
In the center of the tube
The fluid will be moving at the same speed in all parts of the tube
None of the above
All of the following are true of gases except:
Volume and pressure are inversely proportional
Temperature is inversely proportional to volume
Volume is directly proportional to temperature
Volume is directly proportional to the # of moles
The equation for showing the relationship between pressure and volume of gases is:
P1/V1=P2/V2
V1/P1=V2/P2
P1V1=P2V2
P1+V1=P2+V2
As pressure of a gas increases, the volume:
Stays the same as they are not related
Decreases
Increases
Increases by a factor of 2
As temperature increases, volume:
Increases
Decreases
Stays the same
STP describes:
Standard temperature and pressure
Standard atmospheric pressure
Statement of temperature proportions
To find volume of a gas, what is the equation:
V=RT/nP
V=nT/PR
V=nRT/P
V=PRT/n
To increase the relative humidity, we can:
Decrease the partial pressure
Increase the vapor pressure
Increase the partial pressure
None of the above
The Kinetic Molecular Theory of Gases includes all of the following except:
There is a high attraction between gas particles causing them to want to stay close to each other
Gases consist of small particles whose volume is negligible compared to the volume of the gas
Gas molecules are in constant motion
Molecules in a sample show a range of kinetic energies but the average depends only on the temperature
The average kinetic energy of a gas depends on:
Pressure
Temperature
Velocity
None of the above
The Van der Waals Equation took the Ideal Gas Law and took into account the different what of gases?
Density
KE
Speed
Volume
The three principle intermolecular forces include all of the following except:
Dipolar attractions
Ionic bonding
Hydrogen bonding
London forces
Match the types of bonding: | |
|---|---|
London forces | |
Dipole-dipole attraction | |
Polar covalent bond | |
Ionic bond | |
Ion-dipole attraction | |
Covalent bond | |
Hydrogen bond |
The most important intermolecular force is:
Hydrogen bonding
London Forces
Covalent bonds
Dipolar attractions
All of the following are true of surface tension except:
Molecules in the liquid state are attracted to all neighboring molecules by intermolecular forces
Near the surface, there are many balancing attractions from above the surface of the liquid
Deep in the sample, molecular forces operate in all directions and cancel each other out
The attractive strength on the surface of the liquid is the surface tension
What is capillary rise?
The cohesive forces between the water molecules
The tendency of a fluid to rise into a narrow-diameter tube
The opposite of the meniscus value
The tendency of droplets to form on the lid of a pot that has boiling water
A small tube from a gutter system leads into a larger tube that drains into the sewer. Both tubes have the same flow rate. What is the relationship between the pressure and velocity of these tubes?
Pressure in the smaller tube creates a higher velocity
Pressure in the larger tube is less but the velocity is slower
Pressure in the smaller tube is lower allowing for a higher velocity
The velocity is the same but the pressure in the small tube is higher
All of the following are ways we can increase flow rate of a viscous fluid except:
Increase temperature
Increase area
Increase velocity
Increasing pressure
There are two containers. One has helium. One has hydrogen. The mass of each are identical as well as the temperature. Which has the higher Kinetic Energy?
Hydrogen as it has a smaller molar mass
The KE are the same.
Helium due to the higher speed of particles allowing it to float
Unable to determine with information given
The sum of all mole fractions is equal to:
1
100%
Unable to determine with info given.
None of the above
Which gas has the highest effusion rate?
The one with the largest molecular mass
The one with the highest lipophilicity
The one with the lowest molecule mass
The one with the highest KE
What is the pressure of 5g of helium at a temperature of 36 degrees Celsius. With a volume of 10,000mL
3.2 atm
32 atm
12.6 atm
4.3 atm
In water, what is the force we have to overcome in order to break the surface?
Covalent bonding
Surface tension
Polar covalent bonding
None of the above
What structure does surfactant have?
Lipophilic head, hydrophilic tail
Polar head, nonpolar tail
Hydrophobic head, lipophilic tail
None of the above
Adding salt to water has what effect on the boiling point?
Decreases it
Increases it
No change to boiling point
Not enough information
Adding salt to water has what effect on the freezing point?
Decreases it
Increases it
No change
Not enough info
All of the following are colligatve properties except:
Vapor pressure of a solution increases with increasing solute concentration
The boiling point of a solution increases with increasing solute concentration
The freezing point of a solution decreases with increasing solute concentration
The osmotic pressure of a solution increases with increasing solution concentration
Which is true of vapor pressure:
The greater the intermolecular forces the lower the vapor pressure
Vapor pressure decreases with increased temperature
The greater the intermolecular forces the higher the vapor pressure
Vapor pressure is how gases consensate
Match the questions to what they represent: | |
|---|---|
MRT (Molarity x ideal gas constant x Temperature) | |
χ x P (molar fraction x vapor pressure of that solution) | |
(g of solute/g of solution) x 10^6 | |
Equivalents of solute/Liter of solution (expressed mEq) | |
KH x Pgas (Henry's Law constant x partial pressure of the gas) | |
Mol of solute/L of solution | |
Mol of solute/kg of solvent |
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