green chemistry - udvash
TRANSCRIPT
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Green chemistry
Maximum production Minimum pollution
Atom Economy (AE)
AE = �������� ������� ����
����� ������� ���� ×100
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Math Problem
Titanium can be extracted by two methods :
(i) ���� + 2�� → �� + 2���
(ii) ���� → �� + ��
Which one is greener?
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CFC
Chloro Fluoro Carbon
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Poll question: 01
Chemical formula of CFC-13 is ?
(a) CF2Cl2
(b) CFCl3(c) CCl4(d) CF3Cl
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Reaction rate
A = B A + B = C + D A + 2B = C + D aA + bB = cC + dD
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4NH3(g) + 5O2(g) → 4�� � + 6H2O(g) ; at a certain point NH3 reacts at a rate of 0.24 molL-1s-1
a. Write the rate equation.b. Calculate the rate of water production.
[BUET 17-18]
Math Problem
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Reaction theory
Collision theory Transition state theory
The reactants must collide
Collision must occur with a minimum energy (Activation energy: EA )
Collision must occur with proper orientation
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1. Surface area of reactant
Rate determining factors
2. Temperature
3. Concentration
4. Catalyst
5. Pressure
6. Nature of reactant
7. Presence of light
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Poll question: 02
Which one isn’t a factor of reaction rate?
(a) Temperature
(b) Pressure
(c) Product
(d) Concentration
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Temperature
Arrhenius Equation: � = �������
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If slope of lnk vs T-1 is -100K, calculate the activation energy?
Math Problem
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Rate constant at two different Temp.
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Ativation energy of N2O5 dissociation is 100 kJ/mol . Calculate the ratio of rate constant at 00C ও 250C temperature.
V.V.I. for DU
Math Problem
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Reaction order
This relation with rate and reactant conc. depends on the reaction order
A = B
C – rate C – rate C - rate
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A B
0th 1st 2nd
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Half life , � ��
⁄
Time required for a single reactant reaction to completely converts it’s 50% reactant into product(s).
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0th 1st 2nd
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All in ONE
Order Equation Rate constant Half life, t1/2 Half life, t1/2 Unit of k Completion
0th -��
�� = kc0 k =
�
���
�=
�
2���
�∝ � molL-1s-1
Will be completed
1st -��
�� = kc1
k = �
�ln
�
�����
�=
��2
�constant
s-1 Will not be completed
2nd -��
�� =kc2 k =
�
�
�
�(���) ���
=1
�� ��
�∝
1
� L mol-1s-1
Will not be completed
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Poll question: 03
Rate constant of a reaction is 6.3×10-3 L mol-1s-1 .
Which order is it belong to?
(a) 0th
(b) 1st
(c) 2nd
(d) 3rd
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a. Rate at beginning?
b. Conc of reactant after 5s ?
c. Rate at 5s ?
d. When will reactant conc. become 0.2M ?
e. When will reactant conc. become 0.4M ?
f. When all amount of reactant will be converted to product ?
Rate constant of a 1st order reaction is 6.3×10-3 s-1 and the initial conc. is 0.8M
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Poll question: 04
Time required for 40% completion of a 1st order reaction is 10 min. Time required for 100% completion is ?
(a) 30 min
(b) 25 min
(c) Doesn’t complete
(d) 40 min
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a. When �
�of reactant will be remaining?
b. When 12.5% of reactant will be remaining ?
c. Time required for �
�of reactant converted to product?
d. Time required for 87.5% of reactant converted to product?
Half life of a 1st order reaction is 400s
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Catalyst
Speed up or Slow down a reaction . Will remain unchanged after reaction
1. Positive catalyst
2 �����
����2 ��� + 3 ��
2. Negative catalyst
2 ����
�����2 ��� + ��
3. Auto catalyst 5������ + 2�����+3 ����� → 2 ����� + 10 ��� + 8���
4. Induced catalyst 2 ������ + �� → 2 ������������� + �� → �� ��������2 ������ + ������� + �� → 2 ������ + �������
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Poll question: 05
Which one a positive catalyst doesn’t ?
(a) Lowering activation energy
(b) Speeding up reaction
(c) Accelerating the equilibrium arisen
(d) Change the equilibrium
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Type 01 (Bond energy )
∆H= Bond breakdown – Bond formation
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Calculate heat of the following reaction using the bond dissociation energy data given-CH4 + Cl2 -> CH3Cl + HClBond energy of C-H = 430.532 kJmol-1
Bond energy of Cl-Cl = 242.90 kJmol-1
Bond energy of C-Cl = 328 kJmol-1
Bond energy of H-Cl = 433 kJmol-1
Math Problem
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Type 02 Heat of neutralization (∆Hn)
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a. Why ∆Hn of strong acid and strong base is constant?
b. If one or both of them is weak, what will happen?
c. Though HF is a weak acid , why ∆Hn of HF & NaOH is greater than the constant value? [−68.6 kJ mole��]
Math Problem
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Type 03: Formation enthalpy (∆��) ও Heat of combustion (∆��)
Conditions (∆Hf) : 1 mol product & direct reaction between elements
Conditions (∆Hc) : 1 mol reactant & enough oxygen
∆�=Formation enthalpy of product – Formation enthalpy of reactant
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At std. condition, formation enthalpy of CO� g and H�O l are – 400 kJ and −300 kJ.
If heat of combustion of ethanol is −1400 kJ then calculate the formation enthalpy of ethanol.
Math Problem
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Heat of combustion of CS2, C and S is −1100 �� �����, −400 ������� and − 300 ������� respectively . Calculate the formation enthalpy of CS2
Math Problem
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Type 04 : Equation Based
�� → ��; ΔH = ��
�� → ��; ΔH = ��
�� = −��
1.
�� → ��; ΔH = ��
naA → ���; ΔH = ��
�� = ���
2.
� → �; ΔH = ��
� → �; ΔH = ��
� → �; Δ� = �� + ��
3.
Lavoisier- Laplace law
Hess’s law
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Calculate the heat of combustion of carbon
(i) C s +�
�O� g → CO g ∆H� = −111.0 kJ mol�� [DU’15-16]
(ii) CO g +�
�O� g → CO� g ∆H� = −283.0 kJ mol��
Math Problem
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Some Important Formulas
ΔH = ΔU + ΔW
ΔH = ΔU + P.ΔV
ΔH = ΔU + ΔnRT
Qp = Qv + ΔnRT
∆G = ∆H − T∆S
∆�<0; Spontaneous∆�>0; Nonspontaneous∆�=0; Equilibrium
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