# For a non-stoichiometric reaction 2A + B $\to$ C +D, the following kinetic data were obtained in three separate experiments, all at 298 K.  Initial  Concentration (A)  Initial Concentration (B)  Initial rate of formation of C (mol L-1 S-1)          0.1 M         0.1 M  $1.2×{10}^{-3}$          0.1 M         0.2 M $1.2×{10}^{-3}$          0.2 M         0.1 M  $2.4×{10}^{-3}$ The rate law for the formation of C is: 1. d[C]/dt = k[ A][B] 2. d[C]/dt = k[ A]2[B] 3. d[C]/dt = k[ A][B]2 4. d[C]/dt = k[ A]

Subtopic:  Order, Molecularity and Mechanism |
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For the reaction N2 + 3H2 $\to$ 2NH3, the rate $\frac{\mathrm{d}\left[{\mathrm{NH}}_{3}\right]}{\mathrm{dt}}$= 2 x 10-4 M s-1 .Therefore, the rate $\frac{-\mathrm{d}\left[{\mathrm{N}}_{2}\right]}{\mathrm{dt}}$ is given as:

1. 10-4 Ms-1

2. 104 Ms-1

3. 10-2 sM-1

4. 10-4 sM-1

Subtopic:  Definition, Rate Constant, Rate Law |
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If 'I' is the intensity of absorbed light and 'c' is the concentration of AB for the photochemical process AB + hv→  AB *, the rate of formation of AB * is directly proportional to:

1. c

2. I

3. I2

4. cI

Subtopic:  Definition, Rate Constant, Rate Law |
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Which curve represents zero order reaction?

1.

2.

3.

4.

Subtopic:  Order, Molecularity and Mechanism |
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In a reaction, the rate expression is, rate = K[A][B]2/3[C]0, the order of the reaction is:

1. 1

2. 2

3. 5/3

4. zero

Subtopic:  Order, Molecularity and Mechanism |
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The rate of a reaction get doubles when the temperature changes from 7°C to 17°C. By what factor will it change for the temperature change from 17°C to 27°C?

1. 1.81

2. 1.71

3. 1.91

4. 1.76

Subtopic:  Arrhenius Equation |
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In the Arrhenius equation K = Ae-Ea/RT, the quantity e-Ea/kT is referred as:

1. Boltzmann factor.

2. Frequency factor.

3. Activation factor.

4. None of the above.

Subtopic:  Arrhenius Equation |
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For the elementary step, (CH3)3.CBr(aq) → (CH3)3C+ (aq) + Br- (aq), the molecularity is:

1. Zero

2. 1

3. 2

4. Cannot be ascertained

Subtopic:  Order, Molecularity and Mechanism |
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When ethyl acetate was hydrolysed in pressure of 0.1 N HCl, the rate constant was found to be 5.40 x 10-5 sec-1 . But when 0.1 N H2SO4 was used for hydrolysis, the rate constant was found to be 6.25 X10-5sec-1. Thus, it may be concluded that:

1. H2SO4 is stronger than HCI

2. H2SO4 is weaker than HCl

3. H2SO4 and HCl both have the same strength

4. The data are not sufficient to compare the strength of H2SO4 and HCI

Subtopic:  Definition, Rate Constant, Rate Law | Catalyst |
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The half time of a second order reaction is:

1. Inversely proportional to the square of the initial concentration of the reactants.

2. Inversely proportional to the initial concentration of the reactants.

3. Proportional to the initial concentration of reactants.

4. Independent of the initial concentration of reactants.

Subtopic:  First Order Reaction Kinetics |
72%
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