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Chemistry > Gaseous State > Flashcards

Gaseous State Flashcards

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1
Q

Relation between Pressure and root mean square speed

A

P = mnu*u/3V
(where ‘m’ is mase of 1 molecule, ‘n’ is total no. of molecules and V is volume of container)

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2
Q

Most Probable Speed (alpha)

A

square root of (2RT/M)

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3
Q

Average speed

A

Square root of [{(nv)1 + (nv)2}/n1 + n2]
square root of (8RT/pi*M)

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4
Q

Root mean square speed

A

square root of (3RT/M)

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5
Q

(alpha) : average speed : u

A

square root 2 : square root 8/pi : square root 3
1 : 1.1 : 1.224

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6
Q

Relation between speed, Temperature and Most probable speed for fraction of molecules

A

The most the temperature, the more the speed but alpha (waise toh woh increase hi krti hai but for the fraction of molecules) decreases and vice versa.

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7
Q

Kinetic Energy per mole of a gas ( R/N = Boltzmann constant K )

A

3RT/2 or 3PV/2 [ for n moles : 3RT/2*avogadro no. = 3KT/2]

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8
Q

Pressure and Temperature for real gas

A

P = high
T = low

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9
Q

Compressibility Factor

A

Z = PV/nRT

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10
Q

‘Z’ for ideal gas

A

1

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11
Q

Vander Waal equation

A

(P + an*n/V^2)(V - nb) = nRT
where,
a = force of attraction,
b = volume reserved (4VN)
n = no. of moles

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12
Q

Relation between Repulsive Forces and ‘Z’

A

when Z > 1, repulsive forces dominate

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13
Q

Relation between Repulsive Forces and ‘Z’

A
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14
Q

Critical Temperature

A

Temperature below which a gas can be liquified

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15
Q

Critical Pressure

A

Pressure for critical temperature

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16
Q

Critical Volume

A

Volume on critical temperature

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17
Q

Critical Temperature for gases

A

Elementary Gases : Tc is low
Non Elementary Gases : Tc is high

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18
Q

Relation between ‘a’ and Tc

A

the more the value of ‘a’, the more the value of Tc and the better and easy the liquification

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19
Q

Formula for Tc

A

8a/27Rb

20
Q

Formula for Pc

A

a/27b*b

21
Q

Formula for Vc

A

3b

22
Q

CRITICAL :
Pressure * Volume / Temperature

A

= 3R/8

23
Q

Boyle Temperature

A

Temp. on which a gas acts or becomes an ideal gas

24
Q

Inversion Temperature

A

Temperature below which a gas shows cooling effect and above which it shows heating effect

25
Q

Formula for T(boyle)

A

a/Rb

26
Q

Formula for T(inversion)

A

2a/Rb

27
Q

Weak forces

A

Ion dipole interaction
Ion induced dipole interaction
DIPOLE DIPOLE INTERACTION
DIPOLE INDUCED INTERACTION
LONDON FORCES

28
Q

H-bonding

A

type of dipole dipole interaction

29
Q

Relation between distance between dipole and Interaction Energy of Dipole- Dipole interaction

A

1/r^3 ∝ 1/r^6

30
Q

Vander Waal Forces ∝

A

Atomic Masses ∝ Molecular Masses ∝ 1/branching

31
Q

1 atm =

A

76 cmHg
760 mmHg
760 torrHg
almost equal to 1 bar

32
Q

Manometer

A

when closed :
pressure of the gas is Height gained (h) by the liquid (fundamentally - Hg)

when open :
when liquid rises towards narrow tube :
1 atm + height gained by liquid
when liquid rises towards the gas conc. :
1 atm - height gained by the liquid
THE LIQUID IS GENERALLY Hg

33
Q

If the liquid in manometer is not Hg

A

hρ (mercury) = hρ (given liquid)

34
Q

Varying values of R

A

STP : 0.0821
NTP : 0.0831
Joules : 25/3 or 8.31
Calories : 2

35
Q

Gas Laws

A

Boyle’s Law
Charles’s Law
Pressure Law
Avogadro Law
Dalton’s Law of Partial Pressure
Combined Gas Law
Graham Law of Diffusion Effusion

36
Q

Boyle’s Law

A

Pressure ∝ 1/ Volume
when T and Mass of the gas are constant

PV (initial) = PV (final)

37
Q

Charles’s Law

A

Volume ∝ Temperature (in K)
when Pressure and mass is constant
V/T (initial) = V/T (final)

38
Q

Pressure Law

A

Pressure ∝ Temperature (in K)
when volume and mass is constant
P/T (initial) = P/T (final)

39
Q

Dalton’s Law of Partial Pressure

A

Sum of all partial pressures is total pressure for dry gas whereas, for moist gas, aqueous tension is also added to total pressure of dry gas

Partial Pressure = Total pressure * Mole Fraction of the gas (moles of gas/moles of mixture)

40
Q

diffusion (r) and effusion

A

Diffusion : movement of gas from high concentration to low concentration

Effusion : movement of gas through a pinhole or small opening

41
Q

Graham Law for diffusion and effusion

A
42
Q

Graham Law

A

r ∝ P/(density)^2

r1/r2 = P1/P2 * (d2/d1)^2
or
r1/r2 = P1/P2 * (M2/M1)^2

43
Q

Formulae for Rate of Diffusion

A

r = Volume of gas diffused / time
r = Distance travelled by diffused gas / time
r = no. of moles of gas diffused/ time

44
Q

Avogadro Law

A

If two gases have same pressure, volume and temperature, their no. of molecules are equal.

45
Q

(Gay Lussac Law)

A

If reactants and products exist in gases having same temperature and pressure, then for the gas :
Molar Ratio = Volume Ratio

46
Q

Combined Gas Law

A

P1V1/T1 = P2V2/T2

Chemistry (3 decks)

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