The Gas Phase Flashcards

1
Q

Four Gas Variables

A
  • Pressure (P)
  • Temperature (T)
  • Volume (V)
  • Number of moles (n)
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2
Q

Unit(s) of Pressure

A

Pressure = atm, mmHg, torr, kPa

Note:
[1 atm = 760 mmHg = 760 torr = 101.325 kPa]

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3
Q

Unit(s) of Temperature

A

Temperature = K

Note:
273 + C = K
K - 273 = C

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4
Q

Unit(s) of Volume

A

Volume = L or mL

Note:
1 L = 1000 mL or 1 x 10^3

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5
Q

Standard Temperature and Pressure

A

STP = 273 K (0 C) @ 1 atm

Used for Gas Law Equations

Note:
@ STP 1 mole of ideal gas = 22.4 L

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6
Q

Ideal Gas

A

A hypothetical gas where molecules do not exert intermolecular forces and do not occupy any volume.

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7
Q

Ideal Gas Law

A

Def.) Describes relationship between P, T, V, and n.

Eq.) PV = nRT

R = 8.314 when P = kPa
R = 8.21E^-2 when P = atm
R = 62.4 when P = mmHg
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8
Q

Ideal Gas Law: Solve for Pressure (P)

A

P = nRT/V

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9
Q

Ideal Gas Law: Solve for Volume (V)

A

V = nRT/P

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10
Q

Ideal Gas Law: Solve for Number of Molecules (n)

A

n = PV/RT

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11
Q

Ideal Gas Law: Solve for Temperature (T)

A

T = PV/nR

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12
Q

Ideal Gas Law: Density

A

d = PM/RT

Note:
d = density
M = molecular weight

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13
Q

Combined Gas Law

A

[P1V1/T1] = [P2V2/T2]

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14
Q

Avogadro’s Principle

A

P and T held constant; shows n and V are directly proportional

n/V = k n1/V1 = n2/V2

Note:

  • increase in n = increase in V
  • decrease in n = decrease in V
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15
Q

Boyle’s Law

A

T and n held constant; shows P and V are inversely proportional

PV = k P1V1 = P2V2

Note:

  • increase in P = decrease in V
  • decrease in P = increase in V
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16
Q

Gay-Lussac’s Law

A

V and n held constant; shows T and P are directly proportional

P/T = k P1/T1 = P2/T2

Note:

  • increase in P = increase in T
  • decrease in P = decrease in T
17
Q

Charles Law

A

P and n held constant; shows T and V are directly proportional.

V/T = k V1/T1 = V2/T2

Note:

  • increase in V = increase in T
  • decrease in V = decrease in T
18
Q

Gas Properties

A
  • Least dense
  • Indefinite volume or shape
  • Easily compressible
  • Homogenous mixtures
  • Same temperature = same kinetic energy
  • Exist at high temperatures and low pressures