For the reaction, \(2 A+B \rightarrow 3 C+D\)

Which of the following is an incorrect expression for the rate of reaction?

1. \(-\frac{d[C]}{{3} d t }\) 2. \(-\frac{d[B]}{d t} \)
3. \(\frac{d[D]}{d t} \) 4. \(-\frac{d[A]}{2 d t}\)
Subtopic:  Definition, Rate Constant, Rate Law |
 90%
From NCERT
AIPMT - 2006
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The following reaction was carried out at 300 K.

2SO2(g)  +  O2(g) →  2SO3(g)

The rate of formation of SO3 is related to the rate of disappearance of O2  by the following expression:

1. -O2t=+12SO3t                           

2. -O2t=SO3t

3. -O2t=-12SO3t                           

4. None of the above.

Subtopic:  Definition, Rate Constant, Rate Law |
 89%
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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 |
 89%
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The correct expression for the rate of reaction given below is:
\(5 \mathrm{Br}^{-}(\mathrm{aq})+\mathrm{BrO}_3^{-}(\mathrm{aq})+6 \mathrm{H}^{+}(\mathrm{aq}) \rightarrow 3 \mathrm{Br}_2(\mathrm{aq})+3 \mathrm{H}_2 \mathrm{O}(\mathrm{l})\)

1. \(\frac{\Delta\left[B r^{-}\right]}{\Delta t}=5 \frac{\Delta\left[H^{+}\right]}{\Delta t} \) 2. \(\frac{\Delta\left[\mathrm{Br}^{-}\right]}{\Delta t}=\frac{6}{5} \frac{\Delta\left[\mathrm{H}^{+}\right]}{\Delta t} \)
3. \(\frac{\Delta[\mathrm{Br^-}]}{\Delta t}=\frac{5}{6} \frac{\Delta\left[\mathrm{H}^{+}\right]}{\Delta t} \) 4. \(\frac{\Delta\left[\mathrm{Br}^{-}\right]}{\Delta t}=6 \frac{\Delta\left[\mathrm{H}^{+}\right]}{\Delta t}\)
Subtopic:  Definition, Rate Constant, Rate Law |
 88%
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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 |
 89%
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For the reaction,

N2O5(g) → 2NO2(g) + \(\frac{1}{2}\)O2(g)

the value of the rate of disappearance of N2O5 is given as 6.25 × 10-3 mol L-1s-1. The rate of formation of NO2 and O2 is given respectively as:

1. 6.25 x 10-3 mol L-1s-1 and 6.25 x 10-3 mol L-1s-1

2. 1.25 x 10-2 mol L-1s-1 and 3.125 x 10-3 mol L-1s-1

3. 6.25 x 10-3 mol L-1s-1 and 3.125 x 10-3 mol L-1s-1

4. 1.25 x 10-2 mol L-1s-1 and 6.25 x 10-3 mol L-1s-1

Subtopic:  Definition, Rate Constant, Rate Law |
 86%
From NCERT
NEET - 2010
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During the formation of ammonia by Haber's process N+ 3H2 → 2NH3, the rate of appearance of NH3 was measured as 2.5 x 10-4 mol L-1 s-1. The rate of disappearance of H2 will be: 

1. 2.5 x 10-4 mol L-1 s-1

2. 1.25 x 10-4 mol L-1 s-1

3. 3.75 x 10-4 mol L-1 s-1

4. 15.00 x 10-4 mol L-1 s-1

Subtopic:  Definition, Rate Constant, Rate Law |
 84%
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For the reaction, \(\mathrm{N}_2+3 \mathrm{H}_2 \rightarrow 2 \mathrm{NH}_3,\) if, \(\frac{d[NH_{3}]}{dt} \ = \ 2\times 10^{-4} \ mol \ L^{-1} \ s^{-1}\), the value of  \(\frac{-d[H_{2}]}{dt}\) would be:

1. \(3 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \) 2. \(4 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \)
3. \(6 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \) 4. \(1 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\)
Subtopic:  Definition, Rate Constant, Rate Law |
 85%
From NCERT
AIPMT - 2009
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The rate constant of a particular reaction has the dimension of frequency. The order of the reaction is: 

1. Zero.                                                     

2. First.

3. Second.                                                 

4. Fractional.

Subtopic:  Definition, Rate Constant, Rate Law |
 80%
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Which of the following statements about the order of reaction is incorrect?

1. Order is not influenced by the stoichiometric coefficient of the reactants.
2. Order of reaction is the sum of power to the concentration terms of reactants to express the rate of reaction.
3. The order of reaction is always a whole number.
4. Order can be determined by experiments only.
Subtopic:  Definition, Rate Constant, Rate Law |
 79%
From NCERT
AIPMT - 2011
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