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Physics - Gr11 > KTG > Flashcards

KTG Flashcards

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1
Q

Boyle’s Law

A

Volume of a given mass of a gas is inversely proportional to its pressure (PV = K)

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2
Q

Charles’ Law

A

Between volume and temperature at constant pressure (V proportional T)

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3
Q

Gay Lussac’s Law

A

Between Pressure and temperature (P proportional to T)

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4
Q

Derive Perfect gas equation

A

PV = nRT
PV = kNT
P1V1/T1 = P2V2/T2

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5
Q

Value of R

A

8.31J / mole

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6
Q

Value of k

A

1.38 * 10^-23

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7
Q

Explain R - P graph

A
  1. For ideal gas R = 8.31 and is constant
  2. For real gases, higher temperature = lower R value
  3. Higher P = Higher R value
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8
Q

Explain P V graph

A
  1. For ideal gas PV curve more to the right (Predicted by Boyle’s Law)
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9
Q

Explain TV graph

A
  1. Higher P has higher value of graph
  2. Explained by Charles’ Law
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10
Q

Postulates of KTG

A
  1. All gases consist of molecules
  2. Size of molecules negligible compared with distance between
  3. Molecules in state of continuuous random motion
  4. Molecules collide with one another
  5. Collisions are perfectly elastic (no forms of attraction)
  6. Between two collisions a molecule moves in a straight path
  7. Collisions are almost instanteous
  8. Density remains uniform throughout
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11
Q

Expression for pressure exerted by gas

A

P = 1/3 * ro * v^2
Note: v here is mean v or rms v
Derive it

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12
Q

Relation between pressure and KE per unit volume

A

P = 2/3 * avg KE per unit volume

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13
Q

Relation between P and KE

A

PV = 2/3 * avg KE

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14
Q

Vrms in terms of density

A

v = root (3P / ro)

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15
Q

Formula of energy for gas

A

E = 3/2 RT {For one mole}
E = 3/2 kT {Per molecule}

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16
Q

v rms formula (in terms of R)

A

v rm = root (3RT / M)

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17
Q

How to calculate pressure in a mercury tube

A

P = h ro g

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18
Q

Derivation of Boyle’s Law, Charles’ Law, Gay Lussac’s Law, etc.

A

Derive it

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19
Q

Average Speed

A

Arithmetic mean of speed of molecules of a gas at a given temperature

20
Q

Root Mean square speed

A

Defined as the square root of the mean of the squares of the speed of the molucles of a gas

21
Q

Most probable speed

A

Speed possessed by the maximum number of molecules in a gas sample at a given temperature

22
Q

Relation between v(rms), v(mean, v(mp)

A

Vrms > V mean > V mp

23
Q

Degrees of freedom

A

Total number of co-ordinaes or independent quantities required to describe completely the position and configuration of the system

24
Q

Degrees of freedom of a system formula

A

3N - k
N is number of particles in system
k is number of independent relations betweeen particles

25
Q

Length of Hg Tube

A

13.6m

26
Q

Value of pressure in Pa at STP

A

P = 1atm = 1.013 * 10^5

27
Q

Mixture of hydrogen and oxygen has volume 2000 cm^3, temp 300K, pressure 100 kPa and mass 0.76g. Find ratio of no. of moles of hydrogen to no. of moles of oxygen in mixture

A

PV = nRT
n = PV / RT = 0.08
n1 +n2 = 0.08
n1(2) +n2(32) = 0.76
Hence, n1/n2 = 3/1

28
Q

Degrees of Freedom of:
1. Rigid Body
2. Monoatomic Gas
3. Diatoomic gas
4. Triatomic Gas (non - linear)
5. Triatomic (linear)

A
  1. 6 (3 translatory and 3 rotational)
  2. 3 (Only translatory)
  3. 5
  4. 6
  5. 7
29
Q

Law of Equipartition of Energy

A

In any dynamical system in thermal equilibrium, the energy is equally distributed among its various degrees of freedom and energy associated with each degree of freedom per molecule is 1/2 kT

30
Q

Law of Equipartition of Energy derivation

A

1/2 mv^2 = 3/2 kT
If v^2 is the mean squared of components vx^2 +vy^2 + vz^2
1/2 mvx^2 + 1/2 mvy^2 + 1/2 mvz^2 = 3/2 kbT
Hence, since 1/2 mvx^2 = 1/2 mvy^2 = 1/2 mvz^2,
Avg. KE per molecule per degree of freedom is 1/2 kT

31
Q

Specific Heats of:
1. Monoatomic
2. Diatomic
3. Triatomic gases

A
  1. Cv = 3/2 RT (Cp = 5/2RT)
  2. Cv = 7/2 RT (Cp = 7/2 RT)
  3. Cv = 3R (Cp = 4R)
    4.
32
Q

Relation between gamma (Cp / Cv) and f

A

gamma = 1 + 2 / f

33
Q

Specific Heat of Solids

A

Molar specific heat of most of the solids at constant volume is equal to 3R

34
Q

Debye Temperature

A

Temperature at which the molar specific heat of a solid at constant volume becomes equal to 3R

35
Q

Specific heat of water (Cv Value)

A

Cv = 9R

36
Q

Mean Free Path

A

The average distance travelled by the molecule between two successive collisions

37
Q

Mean free path factors

A
  1. Proportional to m
  2. Inversely proportional to density
  3. Inversely proportional to d^2
  4. Proportional to absolute temperature
  5. Inversely proportional to Pressure
38
Q

Lambda expression (mean free path)

A

lambda = (kT) / (root 2 * pi * d^2 * P)

39
Q

Calculate number of molecules in 2 * 10^-6 m^3 of a perfect gas at 300K and at a pressure of 0.01m of mercury. Mean KE of a molecule at 300K = 4* 10^-11 J and g = 9.8

A

P = h ro g = 13.6 * 98
1/2 Mv^2 = 3/2 PV = Total KE
Total KE / KE per molecule = 10^8

40
Q

Higher specific heat capacity = (rate of change of temp)

A

Lower rate
Higher specific heat capacity means heat is used for not onloy in KE but also for translational, rotational, etc.

41
Q

A box contains equal number of molecules of hydrogen and oxygen. If there is a fine hole in the box, which gas will leak rapidly?

A

Hydrogen
v proportional to 1/ root (M)

42
Q

Volume at STP

A

22.4 * 10 ^-3 m^3

43
Q

Molecular weight in SI

A

Molecular weight is in grams
Multiply by 10 ^ -3

44
Q

Relation brtween velocity and temperature

A

v2 / v1 = root (T2 / T1)

45
Q

The molecular KE of 1g of helium at 400K is?

A

KE = 3/2 RT
KE = 3/2 * 400 * 8.31 * 1/4
= 12.465 J

Physics - Gr11 (13 decks)

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