22398.For the reaction, N2 + 3H2 → 2NH3, if $\dfrac{\text{d}NH_3}{\text{d}t}$ = 2 × 10–4 mol L–1 s–1, the value of –$\dfrac{\text{d}H_2}{\text{d}t}$ would be
4 × 10–4 mol L–1 s–1
6 × 10–4 mol L–1 s–1
1 × 10–4 mol L–1 s–1
3 × 10–4 mol L–1 s–1
22399.For a reaction $\dfrac{1}{2}$A → 2B, rate of disappearance of 'A' is related to the rate of appearance of 'B' by the expression:
$–\dfrac{\text{d}[A]}{\text{d}t} = \dfrac{\text{d}[B]}{\text{d}t}$
$–\dfrac{\text{d}[A]}{\text{d}t} = 4\dfrac{\text{d}[B]}{\text{d}t}$
$–\dfrac{\text{d}[A]}{\text{d}t} = \dfrac{1}{2}\dfrac{\text{d}[B]}{\text{d}t}$
$–\dfrac{\text{d}[A]}{\text{d}t} = \dfrac{1}{4}\dfrac{\text{d}[B]}{\text{d}t}$
22400.For a first order reaction (A) → Product, the concentration of A changes from 0.1 M to 0.025 M in 40 minutes. The rate of reaction when the concentration of A is 0.01 M is:
1.73 × 10–5 M/min
3.47 × 10–4 M/min
3.47 × 10–5 M/min
1.73 × 10–4 M/min
22401.Consider the reaction, 2A + B → Products. When concentration of B alone was doubled, the half–life did not change. When the concentration of A alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is:
no unit
mol L–1 s–1
s–1
L mol–1 s–1
22402.The rate of reaction between two reactants A and B decreases by a factor of 4 if the concentration of reactant B is doubled. The order of reaction with respect to reactant B is
2
–2
1
–1
22403.For a reaction A + B → C + D if the concentration of A is doubled without altering the concentration of B, the rate gets doubled. If the concentration of B is increased by nine times without altering the concentration of A, the rate gets tripled. The order of the reaction is
2
1
3/2
4/3
22404.In respect of the equation K = A–Ea / RT
e in chemical kinetics, which one of the following statements is correct?
e in chemical kinetics, which one of the following statements is correct?
k is equilibrium constant
A is adsorption factor
Ea is energy of activation
R is Rydberg's constant
22405.The concentration of R in the reaction R → P was measured as a function of time and the following data is obtained
The order of the reaction is
| [R] (molar) | 1.0 | 0.75 | 0.40 | 0.10 |
| t (min) | 0.0 | 0.05 | 0.12 | 0.18 |
The order of the reaction is
first
second
third
zero
22406.A reaction involving two different reactants can never be
Unimolecular reaction
First order reaction
Second order reaction
Bimolecular reaction