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

An incorrect expression for the rate of reaction is:

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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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%
From NCERT
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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 |
 87%
From NCERT
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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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The decomposition of NH3 on a platinum surface is a zero-order reaction. The rates of production of N2 and H2
 will be respectively:
(given ; k = 2.5 × 10–4 mol–1 L s–1 ) 

1. 2.5 x 10-4 mol L-1 s-1 and 5.5 x 10-4 mol L-1 s-1

2. 2.5 x 10-4 mol L-1 s-1 and 7.5 x 10-4 mol L-1 s-1

3. 1.5 x 10-4 mol L-1 s-1 and 4.5 x 10-4 mol L-1 s-1

4. 0.5 x 10-4 mol L-1 s-1 and 3.5 x 10-4 mol L-1 s-1

Subtopic:  Definition, Rate Constant, Rate Law |
 79%
From NCERT
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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 |
 80%
From NCERT
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The rate equation of a reaction is expressed as, Rate = \(k(P_{CH_{3}OCH_{3}})^{\frac{3}{2}}\)

(Unit of rate = bar min-1)

The units of the rate constant will be:

1. bar1/2 min    
2. bar2 min-1    
3. bar-1min-2  
4. bar-1/2min-1

Subtopic:  Definition, Rate Constant, Rate Law |
 77%
From NCERT
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True statement among the following is:

1. The rate of a reaction decreases with the passage of time as the concentration of reactants decreases.
2. The rate of a reaction is the same at any time during the reaction.
3. The rate of a reaction is independent of temperature change.
4. The rate of a reaction decreases with an increase in the concentration of the reactants.
Subtopic:  Definition, Rate Constant, Rate Law |
 70%
From NCERT
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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 |
 69%
From NCERT
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If at a given instant, for the reaction 2N2O→ 4NO2 + O2 rate and rate constant are 1.02 × 10-4  and 3.4 × 10-5 sec -1 respectively, then the concentration of N2O5 at that time will be: 

1. 1.732 

2. 3.0 

3. 1.02 × 10-4 

4. 3.4 × 105 

Subtopic:  Definition, Rate Constant, Rate Law |
 65%
From NCERT
AIPMT - 2001
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