Hydrogenation of vegetable ghee at 250C reduces pressure of H2 from 2 atom to 1.2 atom in 50 minute. The rate of reaction in terms of molarity per second is:

1. 1.09 x 10-6

2. 1.09 x 10-5

3. 1.09 x 10-7

4. 1.09 x 10-8

Subtopic:  First Order Reaction Kinetics |
67%
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A hypothetical reaction, A2 +B2 $\to$ 2AB mechanism as given below;

A2 $⇌$A+ A          ............(Fast)

A+B2 → AB + B   ............(Slow)

A+ → AB         ............(Fast)

The order of the overall reaction is:

1. 2

2. 1

3. 1.5

4. zero

Subtopic:  Order, Molecularity and Mechanism |
55%
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Following mechanism has been proposed for a reaction,

2A+B $\to$D+E

A+B$\to$ C+D    ...(Slow)

A+ C$\to$ E         ...(Fast)

The rate law expression for the reaction is:

1. r = K[A]2[B]

2. r=K[A][B]

3. r= K[A]2

4. r= K[A][C]

Subtopic:  Definition, Rate Constant, Rate Law |
75%
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In gaseous reactions important for the understanding of the upper atmosphere H2O and O react bimolecularly to form two OH radicals. $∆$H for this reaction is 72kJ at 500 K and Ea is 77 kJ mol-1, then Ea for the bimolecular recombination of two OH radicals to form H2O and O is:

1. 3 kJ mol-1

2. 4 kJ mol-1

3. 5 kJ mol-1

4. 7 kJ mol-1

Subtopic:  Arrhenius Equation |
70%
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For a reaction A Product, rate law is $-\frac{d\left[A\right]}{dt}=K\left[A{\right]}_{0}$. The concentration of A left after time t when $t=\frac{1}{K}$ is:

1. $\frac{\left[A{\right]}_{0}}{e}$

2.

3. $\frac{\left[A{\right]}_{0}}{{e}^{2}}$

4. $\frac{1}{\left[A{\right]}_{0}}$

Subtopic:  First Order Reaction Kinetics |
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For an exothermic chemical process occurring in two steps as;

(i) A+B$\to$X(Slow)

(ii) X$\to$AB (Fast)

The progress of the reaction can be best described by:

 1 2 3 4 All of the above.

Subtopic:  Arrhenius Equation |
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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 |
66%
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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 |
84%
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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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