In the reaction,
3Br2(l)+3H2O(l)
The rate of appearance of bromine (Br2) is related to the rate of disappearance of bromide ions:
1.
2.
3.
4.
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
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. | \(-\frac{d[A]}{2 d t}\) |
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.
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
For the chemical reaction the correct option is:
1.
2.
3.
4.
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. | \(1 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\) |
The half-life period of a first-order reaction is 1386 s. The specific rate constant of the reaction is:
1.
2.
3.
4.
During the kinetic study of the reaction, 2A + B\( \rightarrow\)C + D, following results were obtained:
Run |
[A)/ mol L |
[B)/ mol L |
Initial rate of L |
I |
0.1 |
0.1 |
6.0 |
II |
0.3 |
0.2 |
7.2 |
III |
0.3 |
0.4 |
2.88 |
IV |
0.4 |
0.1 |
2.40 |
Based on the above data which one of the following is correct?
1. rate= k[A]2[B]
2. rate= k[A][B]
3. rate= k[A]2[B]2
4. rate= k[A][B]2
The incorrect statement regarding the order of reaction is:
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. |