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DEEPANKAR TULSIANI,
12 years ago
Grade:12
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1 Answers
aakanksha sharma
4 Points
12 years ago
hi deepankar,
ans cannot be d in any case.listen if t1/2 is 20 min then after 40 min. 1/4th of initial amt.will be left.then ans. is a.
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- NEET Questions
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(2)
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(4)
Subtopic: First Order Reaction Kinetics |
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Rate equation for a second order reaction is:
1. K = (2.303/t) log {a/(a-x)}
2. K = (1/t) log {a/(a-x)}
3. K = (1(a)t-1(ao)t)* 1t
4. K = (1/t2) log {a/(a-x)}
(1)
(2)
(3)
(4)
Subtopic: Order,Molecularity and Mechanism |
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For the reaction 2NO2 + F2 → 2NO2F, following
mechanism has been provided,
NO2 + F2 →slow NO2F+F
NO2 + F →fast NO2F
Thus, rate expression of the above
reaction can be written as:
1. r = K[NO2]2[F2]
2. r = K[NO2 ][F2]
3. r = K[NO2]
4. r = K[F2]
(1)
(2)
(3)
(4)
Subtopic: Definition, Rate Constant, Rate Law |
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For the reaction:
[Cu(NH3)4]2+ + H2O⇌[Cu(NH3)3H2O]2+ + NH3
the net rate of reaction at any time is given by, net rate =
2.0x10-4 [Cu(NH3)4]2+[H2O] - 3.0x105 [Cu(NH3 )3 H20]2+[NH3]
Then correct statement is/are :
1. rate constant for forward reaction = 2 x 10-4
2. rate constant for backward reaction = 3 x 105
3. equilibrium constant for the reaction = 6.6 x 10-10
4. all of the above
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Subtopic: Definition, Rate Constant, Rate Law |
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Rate constant of reaction can be expressed by Arrhenius equation as,
K= Ae-EaRT
In this equation, Ea represents:
1. the energy above which all the colliding molecules will react
2. the energy below which colliding molecules will not react
3. the total energy of the reacting molecules at a temperature, T
4. the fraction of molecules with energy greater than the activation energy of the reaction
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(2)
(3)
(4)
Subtopic: Arrhenius Equation |
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Consider the chemical reaction,
N2g+3H2g→2NH3g
The rate of this reaction can be expressed in terms of time derivative of concentration of N2 g, H2g and NH3g.
The correct relationship amongest the rate expressions is:
(1) Rate =-dN2dt=-13 dH2 dt=12 dNH3dt
(2) Rate =-dN2 dt=-3 dH2dt=2 dNH3dt
(3) Rate =dN2dt=13 dH2dt =12 dNH3dt
(4) Rate =-dN2dt =- dH2dt= dNH3dt
(1)
(2)
(3)
(4)
Subtopic: Definition, Rate Constant, Rate Law |
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For a first order reaction A→ Product, the initial concentration of A is 0.1 M and after 40 minute it becomes 0.025 M. Calculate the rate of reaction at reactant concentration of 0.01M:
1. 3.47x10-4 M min-1
2. 3.47x10-5 M min-1
3. 1.735 x 10-6 M min-1
4. 1.735 x10-4 M min-1
(1)
(2)
(3)
(4)
Subtopic: First Order Reaction Kinetics |
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Select the intermediate in the following reaction mechanism:
O3(g) ⇌ O2(g) +O(g)
O(g) +O3(g) → 2O2(g)
1. O3(g)
2. O(g)
3. O2(g)
4. none of these
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(3)
(4)
Subtopic: Definition, Rate Constant, Rate Law |
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NEET 2023 - Target Batch - Aryan Raj Singh
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A reactant with initial concentration 1.386 mol litre-1 showing first order change takes 40 minute to become half. If it shows zero order change taking 20 minute to becomes half under the similar conditions, the ratio, K1/K0 for first order and zero order kinetics will be:
1. 0.5 mol-1 litre
2. 1.0 mol/litre
3. 1.5 mol/litre
4. 2.0 mol-1 litre
(1)
(2)
(3)
(4)
Subtopic: First Order Reaction Kinetics |
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In a first order reaction, the concentration of the reactant is decreased from 1.0 M to 0.25M in 20 minute. The rate constant of the reaction would be:
1. 10min-1
2. 6.931 min-1
3. 0.6931 min-1
4. 0.06931 min-1
(1)
(2)
(3)
(4)
Subtopic: First Order Reaction Kinetics |
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NEET 2023 - Target Batch - Aryan Raj Singh
To view explanation, please take trial in the course below.
NEET 2023 - Target Batch - Aryan Raj Singh
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