Zero Order Reaction
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In $\mathrm{A}$ reaction; $2\mathrm{A}\to \mathrm{Products}$, the concentration of $\mathrm{A}$ decreases from $0.5\mathrm{mol}{\mathrm{L}}^{-1}\mathrm{to}0.4\mathrm{mol}{\mathrm{L}}^{-1}$ in 10 minutes. Calculate rate during this interval.
The major product $\left[\mathrm{C}\right]$ of the following reaction sequence will be:
The decomposition of NH3 on platinum surface is zero order reaction. What are the rates of production of N_2 and H_2 if k=2.5×10−4 mol−1 Ls−1 ?
For a general reaction A → B , the plot of concentration of A vs time is given in the figure. Answer the following questions on the basis of this graph. (i) What is the order of the reaction? (ii) What is the slope of the curve? (iii) What are the units of rate constant?
103.009≈1020.9
- 25%
- 99.9%
- 75%
- 80%
The rate constant of a first order reaction, whose half-life is 480 seconds, is
1.44 x 10^{-3} s^{-1 }
0.72 x 10^{-3} s^{-1}
2.88 x 10^{-3} s^{-1}
1.44 s^{-1}
For a zero order reaction will the molecularity be equal to zero? Explain.
NO2+F2→2NO2F
Mechanism involves two steps:
I: NO2+F2→2NO2F+F (Slow)
II : NO2+F→NO2F (Fast)
Choose the correct option(s):
- Molecularity of I step is 2
- II is the rate determining step.
- I is the rate determining step.
- Molecularity of I step is 1
यदि एक अभिक्रिया का वेग नियतांक 9.212 × 10^{–4} s^{–1} है, तो अभिक्रिया के 75% पूर्णता के लिए आवश्यक समय होगा
- 10 min
10 मिनट - 15 min
15 मिनट - 20 min
20 मिनट - 25 min
25 मिनट
In the case of a zero-order reaction, the ratio of time required for $75\%$completion to $50\%$ completion is?
The rate constant of the reaction A→B is 0.6×10−3 mole per second. If the concentration of B after 20 min is:
0.36 M
1.08 M
3.60 M
0.72 M
Write the rate equation for the reaction 2A+B⟶C if the order of the reaction is zero.
What is the value of n to the nearest integer?
(Take log102=0.3)
- 2
- 10
- 0.5
- 100
Consider the kinetic data given in the following table for the reaction A + B + C → Product
Ex. No. | [A] | [B] | [C] | Rate of reaction |
1. | $0.2$ | $0.1$ | $0.1$ | $6\times {10}^{-5}$ |
2. | $0.2$ | $0.2$ | $0.1$ | $6\times {10}^{-5}$ |
3. | $0.2$ | $0.1$ | $0.2$ | $1.2\times {10}^{-4}$ |
4. | $0.3$ | $0.1$ | $0.1$ | $9\times {10}^{-5}$ |
When [A] $=0.15$
[B] $=0.25$
[C] $=0.15$
Rate of reaction is $Y\times {10}^{-5}m/s$. Find $\mathrm{Y}$.
In the reaction A + B → Products, if B is taken in excess, then it is an example of
Second order reaction
Zero order reaction
Pseudo first order reaction
First order reaction
- 30 minutes
- 15 minutes
- 7.5 minutes
- 60 minutes
Entropy change : - 549.4J/k mol
Enthalpy of reaction : -1648 x 10^{3 } J/mol
Derive an expression to calculate time required for completion of zero order reaction.
- 230.3 minutes
- 115.15 minutes
- 460.6 minutes
- None of these
aA → product
follows zero order kinetics. The concentration of A with respect to time (t) is given as:
- [A0] = [A]−kt
- [A] = [A0]+kt
- [A] = [A0]−kta
- [A] = [A0]−akt
At high pressure the following reaction is zero order.
2NH3(g)1130K−−−−−−−−−−−→Platinium catalystN2(g)+3H2(g) Which of the following options are correct for this reaction?
(a)Rate of reaction = Rate constant
(b)Rate of the reaction depends on concentration of ammonia
(c)Rate of decomposition of ammonia will remain constant until ammonia disappears completely
(d)Further increase in pressure will change the rate of reaction
- t1/2∝a ; t1/2∝1a
- t1/2∝a ; t1/2∝a0
- t1/2∝a0 ; t1/2∝a
- t1/2∝a ; t1/2∝1a2
Which of the following statements is incorrect about rate of reaction ?
The unit of rate constant is mol L^{-1} s^{-1}
It can be expressed as the rate of decrease in concentration of any one of the reactants.
It can be expressed as the rate of decrease in concentration of any one of the products
It can be expressed as the rate of increase in concentration of any one of the products