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Chemistry Class 11 > Equilibrium > Flashcards

Equilibrium Flashcards

1
Q

Henry’s law

A

Mass of a gas dissolved in a given mass of solvent at any temp is prop to pressure of gas above solvent

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2
Q

Character of equilibrium

A
  1. Possible on in closed system
  2. Both the opposing processes occur at same rate
  3. All measurable qualities remain const
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3
Q

Eq. mixture

A

Mixture of reactants & products in eq state

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4
Q

Eq equation also known as

A

Law of mass action

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5
Q

Law of chemical eq

A

At a temp, product of conc of products raised to their stoichio coeff divided by product of conc of reactants raise to their stoichio coeff is a const

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6
Q

Homogeneous system

A

Reactants & products are in same phase

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7
Q

Delta n =

A

No of moles of (products -reactants)

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8
Q

Features of eq const

A
  1. Applicable only when conc of reactants & products have constant value at eq
  2. Independent of initial conc
  3. Temp dependant
  4. Eq const for Reverse reaction = eq const for forward reaction
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9
Q

Applications of eq const

A
  1. Predict extrnt of reaction based on its magnitude
  2. Predict direction of reaction
  3. Calc eq conc
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10
Q

If K(c) > 10³

A

P > R

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11
Q

If K(c) < 10^-3

A

R > P

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12
Q

If Q(c) > K(c)

A

Dir of R

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13
Q

If Q(c) < K(c)

A

Dir of P

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14
Q

If delta G is -ve

A

Fd dir

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15
Q

Le chatelier’s principle

A

Change in any factor that determine eq of a system will cause the system to change to reduce & counteract the change

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16
Q

Effect of pressure change on eq

A

A pressure change obtained by changing volume can affect yield of products where total no of moles of reactants & products are diff

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17
Q

If volume is halved, partial pressure & conc

A

Doubles

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18
Q

Effect of inert gas

A

Addition of it at const volume doesn’t change Laotian pressure or conc

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19
Q

Eq const for exothermic when temp increases

A

Decreases(-ve delta H)

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20
Q

Effect if catalyst

A

No effect

21
Q

Ionic eq

A

Eq btw ions & unionized molecules

22
Q

Dissociation

A

Separation of ions in water already existing in solid state of solute

23
Q

Arrhenius concept of acids & bases

A

Acids dissociate in water to give H+ & bases OH‐

24
Q

Conjugate acid-base pair

A

Acid-base pair that differs only by 1 proton

25
Q

Bronsted Lowry theory

A

Acids are capable of donating H+ & bases accepting H+

26
Q

Bronsted acid is strong when

A

It’s conjugate base is weak

27
Q

Lewis acids & bases

A

Acids accepts e’ pair & bases donates e’ pair

28
Q

Stronger acid ___ to stronger base

A

Donates a proton

29
Q

K(w)

A

Ionic product of water
K(w) = [H+][OH-] = 10^-14M²

30
Q

K(w) is ___ dependant

A

Temp

31
Q

pH of a solution

A

-log[H+]

32
Q

Dissociation/ionization const

A

K(a)

33
Q

__ the value of K(a) stronger the acid

A

Larger

34
Q

Base ionization const

A

Eq const for base ionization

35
Q

K(b) =

A

c@²/(1-@)

36
Q

K(net) =

A

K1 × K2 ×…

37
Q

__ × __ = K(w)

A

K(a) × K(b)

38
Q

Polyprotic acids

A

Acids that have > 1 ionizable proton per molecule

39
Q

Extent of dissociation of acid depends on

A

Strenth & polarity of H-A bond

40
Q

When strength of H-A bond ___, energy to break it ___ so HA becomes stronger acid

A

Decreases; decreases

41
Q

Acid strength in increasing order

A

HF«HCL«HBr«HI

42
Q

E’ -vity of A in increasing order

A

CH4<NH3<H20<HF

43
Q

Common ion effect

A

Shift in eq on adding a sub that provides more of an ionic species already present in dissociation eq

44
Q

Buffer solution

A

Solutions which resist change in pH on addition of small amounts

45
Q

Henderson-Hasselbalch equation for acid

A

pH = pKa + log[Conj base,A-]/[Acid,HA]

46
Q

Henderson-Hasselbalch equation for base

A

pOH = pKb + log[Conj acid,BH+]/[base,B]

47
Q

pH = pKa +

A

log[Salt]/[Acid]

48
Q

Henderson equation for acid & base together

A

pH = pKa + log[Conj acid, BH+]/[Base,B]

49
Q

Solvation enthalpy is always

A

-ve

Chemistry Class 11 (9 decks)

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