The correct statement about the rate constant of a reaction is:

1. Rate constant is nearly doubled with a rise in temperature by 10 °C 
2. Rate constant becomes half with a rise in temperature by 10 °C 
3. Rate constant remains unchanged with a rise in temperature by 10 °C 
4. None of the above

Subtopic:  Arrhenius Equation |
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The average rate of reaction between the time interval of 30 to 60 seconds in the below mentioned pseudo 1st order reaction is:
t/s 0 30 60 90
[Ester]/mol L-1 0.55 0.31 0.17 0.085

1. 6.67 ×10-2 mol L-1 s-1
2. 2.67 × 10-4 mol L-1 s-1 
3. 4.67 × 10-3 mol L-1 s-1
4. 4.27 × 103 mol L-1 s-1

Subtopic:  Definition, Rate Constant, Rate Law |
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A reaction is first-order with respect to A and second-order with respect to B. The concentration of B is increased three times. The new rate of the reaction would:

1. Decrease 9 times 2. Increase 9 times
3. Increase 6 times 4. Decrease 6 times
Subtopic:  Definition, Rate Constant, Rate Law |
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In a reaction between A and B, the initial rate of reaction (r0) was measured for different initial concentrations of A and B as given below:

A / mol L-1 0.20 0.20 0.40
B / mol L-1 0.30 0.10 0.05
ro / mol L-1 s-1 5.07 x 10-5 5.07 x 10-5 1.43 x 10-4


The order of the reaction with respect to A and B would be:

1. The order with respect to A is 0.5 and with respect to B is zero.
2. The order with respect to A is 1 and with respect to B is 0.5
3. The order with respect to A is 2 and with respect to B is 1
4. The order with respect to A is 1.5 and with respect to B is zero

Subtopic:  Definition, Rate Constant, Rate Law |
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For a reaction, 2A + B C + D, the following observations were recorded:

Experiment [A]/mol L-1 [B]/mol L-1 Initial rate of formation
of D/mol L-1 min-1
I 0.1 0.1 6.0 x 10-3
II 0.3 0.2 7.2 x 10-2
III 0.3 0.4 2.88 x 10-1
IV 0.4 0.1 2.40 x 10-2

The rate law applicable to the above mentioned reaction would be:

1. Rate = k[A]2[B]3

2. Rate = k[A][B]2

3. Rate = k[A]2[B]  

4. Rate = k[A][B]  

Subtopic:  Definition, Rate Constant, Rate Law |
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Given the following observations:

Experiment [A] / mol L-1 [B] / mol L-1 Initial rate / mol L-1 min-1
I 0.1 0.1 2.0 x 10-2
II X 0.2 4.0 x 10-2
III 0.4 0.4 Y


The reaction between A and B is first-order with respect to A and zero-order with respect to B. The values of X and Y are, respectively:

1.  X = 0.2 \(mol\) \(L^{- 1}\); Y = \(\) \(0 . 08\) \(mol\) \(L^{- 1} \left(min\right)^{- 1}\)

2.  X = 0.02 \(mol\) \(L^{- 1}\); Y = \(\) \(0 . 08\) \(mol\) \(L^{- 1} \left(min\right)^{- 1}\)

3.  X = 0.01 \(mol\) \(L^{- 1}\); Y = \(\) \(0 . 8\) \(mol\) \(L^{- 1} \left(min\right)^{- 1}\)

4. X = 0.2 \(mol\) \(L^{- 1}\); Y = \(\) \(0 . 8\) \(mol\) \(L^{- 1} \left(min\right)^{- 1}\)

Subtopic:  First Order Reaction Kinetics |
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The rate constant of a radioactive substance is 4 years-1. The value of half-life will be : 

1. 0.05 years

2. 0.17 years

3. 0.26 years-1

4. 1.6 years

Subtopic:  First Order Reaction Kinetics |
 86%
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During a nuclear explosion, one of the products is 90Sr with a half-life of 28.1 years. If 1µg of 90Sr was absorbed in the bones of a newly born baby instead of calcium, the amount of 90Sr that will remain after 10 years in the now grown up child would be -

(Given ,antilog(0.108)=1.28)

1. 0.227 µg 

2. 0.781 µg 

3. 7.81 µg 

4. 2.27 µg 

Subtopic:  First Order Reaction Kinetics |
 67%
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For the decomposition of azoisopropane to hexane and nitrogen at 543 K, the following data was obtained:

4l

The rate constant of the above reaction would be -

1. 1.21 x 10-3 s-1

2. 2.21 x 10-3 s-1

3. 3.21 x 10-3 s-1

4. 4.21 x 10-3 s-1

Subtopic:  First Order Reaction Kinetics |
 60%
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For the  reaction 2A + BA2B, rate = kAB2 with k = 2.0×10-6 mol-2L2s-1 and A=0.1 M; B=0.2 M. The initial rate of the reaction will be :

1. 0.04×10-9 mol L-1 s-1

2. 8×10-8 mol-1L s-1

3. 8×10-9 mol L-1 s-1

4. 8×10-7 mol L-1 s-1

Subtopic:  Definition, Rate Constant, Rate Law |
 74%
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