The decomposition of N2O5 in CCl4 at 318K has been studied by monitoring the concentration of N2O5 in the solution. Initially, the concentration of N2O5 is 2.33 mol L–1 and after 184 minutes, it is reduced to 2.08 mol L–1. The reaction takes place according to the equation

2 N2O5 (g)  4 NO2 (g) + O2 (g)

The rate of production of NO2 during this period is-

1. 5.72 × 10
–3 mol L–1 min–1
2. 2.72 × 10
–3 mol L–1 min–1
3. 1.72 × 10
–5 mol L–1 min–1
4. 6.72 × 10
–4 mol L–1 min–1
 

Subtopic:  Definition, Rate Constant, Rate Law |
 65%
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Consider the two rate laws:

(I) Rate = k [A]1/2 [B]3/2

(II) Rate = k [A]3/2 [B]–1

The correct statement among the following is-
 

1. The overall order for rate expression (I) is 2 and for (II) is \(\frac{5}{2}\).
2. The overall order for rate expression (I) is 2 and for (II) is \(\frac{1}{2}\).
3. The overall order for rate expression (I) is -2 and for (II) is \(\frac{3}{2}\).
4. The overall order for rate expression (I) is -2 and for (II) is \(\frac{5}{2}\).




 

Subtopic:  Order, Molecularity and Mechanism |
 92%
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Consider the following values of rate constant:

(i) k = 2.3 × 10–5 L mol–1 s–1

(ii) k = 3 × 10–4 s–1

The correct statement among the following is-

1. The order for (i) is second order and the order for (ii) is first order.
2. The order for (i) is zero order and the order for (ii) is first order.
3. The order for (i) is second order and the order for (ii) is zero order.
4. The order for (i) is first order and the order for (ii) is zero order.




 

Subtopic:  First Order Reaction Kinetics |
 75%
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The initial concentration of N2O5 in the following first-order reaction N2O5(g)  2 NO2(g) + 1/2 O2 (g) was 1.24 × 10–2 mol L–1 at 318 K. The concentration of N2O5 after 60 minutes was 0.20 × 10–2 mol L–1. The rate constant value at 318 K is-

 1. 0.304 min
-1
2.
0.00304 min-1
3. 0.0304 min-1
4. 3.04 min-1

Subtopic:  First Order Reaction Kinetics |
 62%
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The following data were obtained during the first order thermal decomposition of N2O5 (g) at constant volume:

2N2O5(g) 2N2O4(g) + O2(g)
 

  S.NO.  Time/s  Total Pressure/(atm)
  1   0    0.5
  2   100    0.512


The rate constant value is-

1. \(5.98\times 10^{-4}\) sec-1
2. \(4.98\times 10^{-4}\) sec-1
3. \(6.98\times 10^{-4}\) sec-1
4. \(7.98\times 10^{-4}\) sec-1

Subtopic:  First Order Reaction Kinetics |
 63%
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A first-order reaction is found to have a rate constant, = 5.5 × 10-14 s-1. The half-life of the reaction is-

1.
1.66 × 1013 s
2.  1.46 × 1013 s
3. 1.36 × 1013 s
4. 1.26 × 1013 s



 

Subtopic:  First Order Reaction Kinetics |
 80%
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In a first order reaction, time required for completion of 99.9% is X times of half-life (t1/2) of the reaction. When reaction is completed 99.9%, [R]n = [R]0 – 0.999[R]0 .The value of X is-

1. 5
2. 10
3. 15
4. 20

Subtopic:  First Order Reaction Kinetics |
 80%
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The rate constants of a reaction at 500K and 700K are 0.02s–1 and 0.07s–1 respectively. The values of Ea is-

1. 15.6 kJ
2. 13.7 kJ
3. 18.2 kJ
4. 17.5 kJ

Subtopic:  First Order Reaction Kinetics |
 53%
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The first-order rate constant for the decomposition of ethyl iodide by the reaction

C2H5I(g)  C2H4 (g) + HI(g)

at 600K is 1.60 × 10–5 s–1. Its energy of activation is 209 kJ/mol. The rate constant of the reaction at 700K is-

1. 7.56 × 10
–3 s–1
2.
6.36 × 10–3 s–1
3. 5.16 × 10–3 s–1
4. 5.76 × 10–3 s–1

Subtopic:  Arrhenius Equation |
 56%
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The rate constants of a reaction at 500K is 0.02s–1 . The values of Ea is 18.230 kJ. The value of A is-

1. 1.61
2. 1.41
3. 1.81
4. 1.21


 
Subtopic:  Arrhenius Equation |
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