The rate constant (in mol L⁻¹ s⁻¹) for a zero-order reaction with an initial concentration of 0.02 M and a half-life of 100 seconds is:

1. \(1.0 \times 10^{-4}\)
2. \(2.0 \times 10^{-4}\)
3. \(2.0 \times 10^{-3}\)
4. \(1.0 \times 10^{-2}\)

Subtopic:  Definition, Rate Constant, Rate Law |
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The temperature dependence of rate constant (k) of a chemical reaction is written in terms of Arrhenius equation, = Ae-Ea/RT . Activation energy Ea of the reaction can be calculated by plotting : 

(1) log vs 1 / log T

(2) k vs T

(3) k vs 1 / log T

(4) log k vs 1 / T

Subtopic:  Arrhenius Equation |
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If the rate of the reaction is equal to the rate constant, the order of the reaction is : 

(1) 3

(2) 0

(3) 1

(4) 2

Subtopic:  Definition, Rate Constant, Rate Law |
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3A  B + C

It would be a zero order reaction when :

(1) The rate of reaction is proportional to square of concentration of A

(2) The rate of reaction remains same at any concentration of A

(3) The rate remains unchanged at any concentration of B and C

(4) The rate of reaction doubles if concentration of B is increased to double.

Subtopic:  Definition, Rate Constant, Rate Law |
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The activation energy for a simple chemical reaction
B is Ea in the forward direction.
The activation energy for the reverse reaction:

1. Can be less than or greater than Ea

2. Is always double of Ea

3. Is negative of Ea

4. Is always less than Ea

Subtopic:  Arrhenius Equation |
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For a chemical reaction A product, the postulated mechanism of the reaction is as follows.

Ak2k13BR.D.Sk3C
If the rate constants for individual reactions are  k1, k2 and k3, and activation energies are 
\(E_{a_{1}} = 180 \ kJ \ mol^{-1}, \)
\( E_{a_{2}} = 90 \ kJ \ mol^{-1}, \)
\( E_{a_{3}} = 40 \ kJ \ mol^{-1}\)
then overall activation energy for the reaction given above is

1. 70 kJ mol-1

2. -10 kJ mol-1

3. 310 kJ mol-1

4. 130 kJ mol-1

Subtopic:  Arrhenius Equation |
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The reaction below is an example of:

CH3COOC2H5   +   H2O   \(\xrightarrow[]{H^{+}}\) CH3COOH  +   C2H2OH
Ethyl acetate                           Acetic acid     Ethyl alcohol



1. Pseudo-first-order reaction

2. First-order reaction

3. Second order reaction

4. Third-order reaction

Subtopic:  Order, Molecularity and Mechanism |
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What is the rate equation for reaction 2A+ B C if the order of the reaction is zero ?

1. k [A]0 [B]0

2. k [A]1[B]0

3. k [A]1[B]1

4. None of these

Subtopic:  Order, Molecularity and Mechanism |
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For a certain reaction large fraction of molecules have energy more than the threshold energy, yet why the rate of reaction is very slow.It is due to improper: 

1. Orientation of colliding molecules.

2. Energy of colliding molecules.

3. Volume of colliding molecules.

4. Entropy of colliding molecules.

Subtopic:  Arrhenius Equation |
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For a general reaction A  B, the plot of the concentration of A vs. time is given in the figure.
 

The slope of the curve will be:

1. -k 2. -k/2
3. -k2 4. -k/3
Subtopic:  Definition, Rate Constant, Rate Law |
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