Chapter 8: The Gas Phase Flashcards
If you had a balloon filled with helium tied and suspended in a vehicle, and the vehicle accelerated, which way would the balloon travel?
The balloon would travel in the same direction of the acceleration, which is counterintuitive. If accelerating forward, the helium filled balloon will move forward because the density of the helium (4 g/mol) is less than that of the surrounding air (29 g/mol). Given that the air has more density, the air has greater inertia than the helium and resists the forward motion more than the helium, shifting the air backward and causing the helium to shift forward. Super cool example.
What is the normal adult blood pressure?
Less than 120mmHg systolic/ 80mmHg diastolic.
Hypertension is having at least two blood pressures exceeding the 140/90.
What is standard temperature and pressure (STP)? Recall standard state, what is standard state?
What are the four variables that define the state of a gaseous sample?
What is the SI unit of pressure? What is the relationship between atmospheric pressure, mmHG, torr, and pascal?
Compare and contrast STP and standard state conditions.
They both refer to temperatures and pressures, but have different purposes.
STP is 273 K and 1 atm and generally used for gas law calculations.
Standard state conditions are generally 298K, 1 atm, at 1M concentrations (1mol/L), and are used when measuring standard enthalpy, entropy, free, energy, changes, and electrochemical cell voltage.
Name some characteristics that make the gas phase unique.
Gases are compressible fluids with rapid molecular motion, large intermolecular distances, and weak intermolecular forces.
Concept check page 280 gas phase:
What are the assumptions made for an ideal gas?
An ideal gas represents a hypothetical gas with molecules that have no intermolecular forces and occupy the volume.
Although real gases deviate from this ideal behavior at high pressures, low volume, and low temperatures, many compressed gases demonstrate behavior that is close to ideal.
What is the ideal gas law?
What are the different expressions of the ideal gas law (hint: SI units)?
Why is it important to know the different expressions of the ideal gas law?
What is does one joule represent?
What does one newton represent?
What is the ideal gas constant used to do?
What does the graph of P and V look like for given temperatures of an ideal gas when n, R, and T are held constant?
Example page 282, ideal gas law:
What is density defined as? What is the usual expression for density of a gas?
What is the equation for density of a gas? How can we rearrange the ideal gas law to calculate the density of a gas?
What is the combined gas law? How is it used?
How can we calculate a change in volume and density under non standard conditions given the combined gas law?
Gas density example page 283:
What volume does one mole of an ideal gas at STP occupy?
At STP (273 k and 1 atm), one mole of ideal gas occupies 22.4 L
How can you determine molar mass of a sample of gas using the ideal gas law?
How can you determine molar mass of a sample of gas using the ideal gas law?
Example from book molar mass calculation of gas page 284:
What are the four laws of the ideal gas law?
Describe Avogadro’s Principle.
Example Avogadro’s principle question page 285:
What is Boyles law? Describe the graph produced with Boyles law.
What is Charle’s Law? Describe the graph of Charle’s law.
Example Charles’s Law page 286:
What is Gay-Lussac’s Law? What is the graph produced by Gay-Lussac’s Law?
Gay-Lussac’s Law example page 288:
What does Daltons Law of Partial Pressures state? What is the equation? How do you determine the partial pressure of a gas in a mixture knowing the total pressure of the mixture?
How do you determine the partial pressure of a gas in a mixture when you know the total pressure of the mixture?
Example Daltons Law of Partial Pressures page 289:
What is Henry’s Law?
Relate the biological importance of Henry’s Law regarding parity’s pressures and solubility.
Henry’s Law example page 291:
Concept check page 291 ideal gases:
Concept check ideal gases page 291
Concept check ideal gas page 291:
Concept check ideal gas page 291:
Concept check ideal gas page 291:
Concept check ideal gas page 292:
Concept check ideal gas page 292
What are the assumptions of the kinetic molecular theory?
What is the equation for kinetic energy of a gas particle according to the kinetic molecular theory of gases?
What is the root mean square speed (u rms)? What does it allow us to calculate?
Describe a Maxwell Boltzmann distribution curve.
Example root mean square speed page 294
What is diffusion? Effusion? What is a pleural effusion?
What is grahams law?
Example grahams law page 296
Concept check kinetic molecular theory page 293:
Concept check kinetic molecular theory page 293:
Concept check kinetic molecular theory page 293:
Concept check kinetic molecular theory page 293:
In what way do real gases differ from ideal gases? When do they differ the most?Describe the isothermal graphs of ideal and real gases.
Which gas will exert a higher pressure under the same, non-ideal conditions:
Methane
Chlromethane
If methane and isobutane are placed in the same size container under the same conditions, which will exert the higher pressure (consider both is having negligible attractive forces)?
If methane and isobutane are placed in the same size container under the same conditions, which will exert the higher pressure (consider both is having negligible attractive forces)?
Describe why real gases behave different ideal.
What is the Van der Walls equation of state? Describe a and b in the corrections, relate the corrections with a and b.
Concept check gas phase page 274 question 1
Concept check gas phase page 274 question 2
Concept check gas phase page 274 question 3
Concept check gas phase page 274 question 4
Concept check gas phase page 274 question 5
Concept check gas phase page 274 question 6
Question 9 page 271 ideal gas
Master question 10 page 275
Mastery question 12 page 275
