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General Chemistry 1 > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

what is pressure?

A

a measure of force exerted per unit area; in chemistry, most commonly the force exerted by gas molecules as they strike the surface around them

P= F/A ( pressure can be measured in several different units)

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2
Q

what is the unit millimeter of mercury (mmHg) aka Torr?

A

a common unit of pressure referring to the air required to push a column of mercury to a height of 1mm in a barometer (760 mmHg = 1 atm = 101.325 kPa)
aka the Torr named after the Italian physicist Evangelista Torricelli

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3
Q

what is a barometer?

A

an instrument used to measure atmospheric pressure

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4
Q

what is the a Pascal?

A

The SI unit of pressure defined as 1 N/m^2

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5
Q

what is an atmosphere?

A

a unit of pressure based on the average pressure of air at sea level; 1 atm = 101 325 Pa)

101 325 Pa = 101.325 kPa = 760 Torr = 1 atm

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6
Q

what is standard pressure?

A

100 000 Pa or 1 bar

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7
Q

what is the bar?

A

a unit of standard pressure that is equal to 100 000Pa

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8
Q

what is a manometer?

A

an instrument used to determine the pressure of a gaseous sample, consisting of a liquid-filled U-shaped tube with one end exposed and the other connected to the sample
(height difference (h) indicates pressure of gas relative to atmospheric pressure)

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9
Q

what is Boyle’s Law?

A

The law that states that the volume of a gas is inversely proportional to its pressure

P1V1 = P2V2

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10
Q

what is Charles law?

A

The law that states that temperature is directly proportional to to its temperature

V1/T1 = V2/T2

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11
Q

what is Avogadro’s Law?

A

The law that states that the volume of a gas is directly proportional to its amount in moles

V1/n1 = V2/n2

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12
Q

what is the Ideal Gas Law?

A

The law that combines the relationships of Boyle’s Law, Charles Law, and Avogadro’s Law into one comprehensive equation of state with the proportionality constant R in the form PV = nRT

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13
Q

what is an ideal gas?

A

a gas that perfectly follows the ideal gas law

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14
Q

what is the ideal gas constant?

A

The proportionality constant of the ideal gas law R, equal to 8.314 J/molK or 0.08314 bar L/molK

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15
Q

what is molar volume?

A

the volume occupied by one mole of a substance

often specified under the conditions known as STP (Standard Temperature and Pressure)

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16
Q

what is STP?

A

The conditions when T = 273.15K and P = 1bar and V = 22.4L

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17
Q

Density of a gas?

A 
since we know the molar volume of an Ideal gas under STP, we can readily calculate the density if a gas under these conditions 
PV = nRT ; n=m/M
PV = (m/M)RT;  d=m/V
m/V = PM/RT
d = PM/RT
18
Q

molar mass of a gas?

A

we can use the ideal gas law in combination with mass measurements to calculate the molar mass of an unknown gas
PV = nRT; n = m/M
PV = (m/M)RT
M = mRT/PV

19
Q

what is partial pressure?

A

the pressure due to any individual component in a gas mixture

20
Q

What is Dalton’s Law of Partial Pressures?

A

The law stating that the sum of the partial pressures of the component gas mixture must equal the total pressure
Ptotal = P(a) + P(b) + ….

P(a)=n(a)RT/Vtotal + P(b) = n(b)RT/Vtotal …= n(total) = RT/Vtotal

21
Q

what is a mole fraction?

A

The number of moles of a component in a mixture divided by the total number of moles in the mixture
X(a) = n(a)/n(total)
P(a) = X(a)P(total)

22
Q

what is hypoxia?

A

A physiological condition caused by low levels of oxygen, marked by dizziness, headache, and shortness of breath and eventually unconsciousness or even death in severe cases

23
Q

what is oxygen toxicity?

A

a physiological condition caused by an increased level of oxygen in the blood, resulting in muscle twitching, tunnel vision and convulsions

24
Q

what is nitrogen narcosis?

A

a physiological condition caused by an increased partial pressure or nitrogen, resulting in symptoms similar to those of intoxication

25
Q

what is Vapour pressure?

A

the partial pressure of a vapour in dynamic equilibrium with its liquid

26
Q

Collecting gas over water?

A

P(total) = P(diatomic gas) + P(H2O)

27
Q

What is the Kinetic Molecular Theory?

A

Average kinetic energy proportional to volume of particle
1. The size of a particle is negligibly small.
2.The average kinetic energy of a particle is proportional to the temperature (in K).
3.Completely elastic collisions between particles
THEORY ASSUMES ALL COLLISIONS ARE ELASTIC, THIS IS NOT A REAL LIFE SCENARIO

28
Q

How does KMT relate to Boyle’s Law

A

as Volume increases, Collisions decrease, and Pressure decreases

29
Q

How does KMT relate to Charles Law?

A

as Temperature increases, Collisions increase, and pressure increases

30
Q

How does KMT relate to Avogadro’s Law?

A

as Moles increase, Collisions increase, and Pressure increases

31
Q

How does KMT relate to Dalton’s Law?

A

as Moles increases, Collisions increases, and Pressure increases

32
Q

Kinetic Molecular Theory and Ideal Gas Law?

A

P = F(total)/A(area)
F(collision) = m(velocity/t) = m(2velocity/t)
#of collisions = (velocitytA)(n/V)
P = (m*velocity^2)(n/V)

33
Q

Temperature and its relation to Molecular velocities

A
  • speed will depend on the weight of a particle
  • particles of different mass will have the same kinetic energy at a given temperature Ek = 0.5mv^2
    -In a gas at a given temperature, lighter particles travel faster (on average) than heavier ones
    u(rms) = √u^2 = √3RT/M
34
Q

what is u(rms)

A

is the speed of a particle, represents an average of all speeds

35
Q

what does mean free path mean?

A

The average distance a molecule in a gas travels between collisions

36
Q

what is diffusion?

A

The process by which a gas spreads through a space occupied by another gas

37
Q

what is effusion?

A

The process by which a gas escapes from a container into a vacuum through a small hole

Rate of effusion = 1/√M
Rate of effusionS = ΔV/Δt

38
Q

what is Graham’s law of effusions?

A

the expression of the ratio of of rates of effusion of two different gases

Rate(a)/Rate(b) = Rate of effusionS = √M(a)/M(b)

39
Q

What is Van der Waals equation?

A

The extrapolation of the ideal gas law that considers the effects of intermolecular forces and particle volume in a non-ideal(real gas)

P + a(n/V)^2 * (V - nb) = nRT

40
Q

what is the real gas formula compared to the ideal gas formula?

A

Ideal Gas = V = nRT/P
Real Gas = V = nRT/P + nb(bar)

V(ideal) = V(real) - nb

41
Q

what is the correction in the real gas formula from the ideal gas formula for particle volume?

A

nb

42
Q

what is the correction in the Van der Waals formula from the ideal gas formula for intermolecular forces?

A

(n/V)^2

General Chemistry 1 (11 decks)

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