Rate of Reaction
Trending Questions
Q. For an elementary chemical reaction, 
the expression for d[A]dt is

the expression for d[A]dt is
- 2k1[A2]−2k−1[A]2
- k1[A2]−k−1[A]2
- k1[A2]+k−1[A]2
- 2k1[A2]−k−1[A]2
Q. For the reaction 2A + B + C →A2B + C the rate law is found to be Rate =k[A][B]2 with k=2×10−6mol−2L2s−1
The initial rate of reaction with [A]=0.1molL−1, [B]=0.2molL−1 and [C]=0.8molL−1 is
The initial rate of reaction with [A]=0.1molL−1, [B]=0.2molL−1 and [C]=0.8molL−1 is
- 8×10−9molL−1s−1
- 6.4×10−8molL−1s−1
- 4×10−7molL−1s−1
- 4×10−3molL−1s−1
Q. Nitrogen tetra oxide (N2O4) decomposes as N2O4(g)→2NO2(g). If the pressure of (N2O4) falls from 0.50 atm to 0.32 atm is 30 minutes, the rate of appearance of NO2(g) is
- 0.006 atm/min
- 0.003 atm/min
- 0.012 atm/min
- 0.024 atm/min
Q. The concentration of a reactant changes from .03M to .02M in 25 minutes. The average rate of reaction, using time in seconds is
- 6.67×10−6mol/l/s
- 0.4×10−3mol/l/s
- 0.024mol/l/s
- 0.24mol/l/s
Q. The data for the reaction is A + B →C is
Exp.[A]0[B]0Initial rate10.0120.0350.1020.0240.0350.8030.0120.0700.1040.0240.0700.80
Exp.[A]0[B]0Initial rate10.0120.0350.1020.0240.0350.8030.0120.0700.1040.0240.0700.80
- r=k[B]3
- r=k[A]3
- r=k[A][B]4
- r=k[A]2[B]2
Q. The rate of a reaction is expressed in different ways as follows:
12(d[C]dt)=−13(d[D]dt)=14(d[A]dt)=−(d[B]dt)
The reaction is
12(d[C]dt)=−13(d[D]dt)=14(d[A]dt)=−(d[B]dt)
The reaction is
- 4A+2B→2C+3D
- B+(1/2)D→4A+3C
- 4A+B→2C+3D
- B+3D→4A+2C
Q. A reaction follows the given concentration (M)-time graph. The rate for this reaction at 20 seconds will be


- 4×10−3M/s
- 8×10−2M/s
- 2×10−2M/s
- 7×10−3M/s
Q. xA+yB→zC.If−d[A]dt=−d[B]dt=1.5d[C]dt then x.y and z are
- 1, 1, 1
- 3, 2, 3
- 3, 3, 2
- 2, 2, 3
Q. In the following reaction, how is the rate of appearance of product related to the rate of disappearance of the reactant?
BrO−3(aq)+5Br−1(aq)+6H+→3Br2(l)+2H2O(l)
BrO−3(aq)+5Br−1(aq)+6H+→3Br2(l)+2H2O(l)
- d[Br2]dt=−d[Br−]dt
- d[Br2]dt=35d[Br−]dt
- d[Br2]dt=−35d[Br−]dt
- d[Br2]dt=−53d[Br−]dt
Q. The rate at which a substance reacts depends upon:
- Atomic weight
- Atomic number
- Molecular weight
- Active mass