A first-order reaction has a rate constant of 2.303 . The time required for 40 g of this reactant to reduce to 10 g will be
[Given that ]
1. | 230.3 s | 2. | 301 s |
3. | 2000 s | 4. | 602 s |
For a reaction, activation energy and the rate constant at 200 K is 1.6 . The rate constant at 400K will be [Given that gas constant, R=8.314 J ]
1. 3.2 × 104 s-1
2. 1.6 × 106s-1
3. 1.6 × 103 s-1
4. 3.2 × 106 s-1
For the chemical reaction the correct option is:
1. | 2. | ||
3. | 4. |
If the rate constant for a first order reaction is k, the time (t) required for the completion of 99% of the reaction is given by:
1. t = 2.303/k
2. t = 0.693/k
3. t = 6.909/k
4. t = 4.606/k
Consider the reaction
N2(g) + 3H2(g) → 2NH3(g)
The equality relationship between \(
\frac{{d}\left[{{NH}_{3}}\right]}{dt}\) and \(
{-}\frac{{d}\left[{{H}_{2}}\right]}{dt}\) is :
1.
2.
3.
4.
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. | \(-\frac{d[A]}{2 d t}\) |
If 60% of a first-order reaction was completed in 60 min, 50% of the same reaction would be completed in approximately:
(log 4 = 0.60, log 5 = 0.69)
1. | 50 min | 2. | 45 min |
3. | 60 min | 4. | 40 min |
In a first order reaction A \(\overset{ }{\rightarrow}\) B, if k is rate constant and initial concentration of the reactant A is 0.5 M then the half-life is :
(1) \(\frac{0 . 693}{0 . 5 k}\)
(2) \(\frac{log 2}{k}\)
(3) \(\frac{log 2}{k \sqrt{0 . 5}}\)
(4) \(\frac{ln 2}{k}\)
The reaction of hydrogen and iodine monochloride is given as:
H2(g) + 2ICl(g) → 2HCl(g) + I2(g)
This reaction is of first order with respect to H2(g) and ICl(g), for which of the following proposed mechanisms:
Mechanism A:
H2(g) + 2ICl(g) → 2HCl(g) + I2(g)
Mechanism B:
H2(g) + ICl(g) →HCl(g) + HI(g); slow
HI(g) + ICl(g) →HCl(g) + I2(g); fast
1. B Only
2. A and B both
3. Neither A nor B
4. A only
The bromination of acetone occurring in an acid solution is represented by the equation.
CH3COCH3(aq)+ Br2(aq) →
CH3COCH2Br(aq) + H+(aq) + Br-(aq)
The kinetic energy data were obtained for given reaction concentrations.
Initial concentrations, M
0.30 0.05 0.05
0.30 0.10 0.05
0.30 0.10 0.10
0.40 0.05 0.20
Initial rate, the disappearance of Br2, Ms-1
5.7 10-5
5.7 10-5
1.2 10-4
3.1 10-4
Based on the above data, the rate of the equation is:
1.
2.
3.
4.