Rate Constant
Trending Questions
The rate of a first order reaction is 0.04mol/L/s at10minutes and 0.03mol/L/s at 20minutes after initiation. Find the half life of the reaction.
 t = 0.693/k
 t = 6.909/k
 t = 4.606/k
 t = 2.303/k
How to calculate the dissociation constant?
What is the relation between half life and average life ?
The following results have been obtained during the kinetic studies of the reaction, 2A+B→C+D
Experiment[A] mol L−1[B] mol L−1Initial rate of formation ofD/mol L−1 minI0.10.16.0×10−3II0.30.27.2×10−2III0.30.42.88×10−1IV0.40.12.40×10−2
Determine the rate law and the rate constant for the reaction.
What is the effect of temperature on the rate constant of a reaction? How can this temperature effect on rate constant be represented quantitatively?
What is the formula to find the flocculation value?
Experiment  [A] (in mol L−1  [B] (in mol L−1)  Initial rate of the reaction (in mol L−1min−1 ) 
(I)  0.10  0.20  6.93x10−3 
(II)  0.10  0.25  6.93x10−3 
(III)  0.20  0.30  1.386x10−2 
 5
 100
 1
 10

7.33
 733
 0.733
 73.3
 Bakelite
 Nylon66
 Terylene
 Neoprene
 2×104
 3.45×10−5
 2×10−4
 1.386×10−4
Molarity of 0.1 N of oxalic acid?
 16×10−3
 64×10−3
 32×10−3
 250
R_{1 }and R_{2 }are two reactions having identical preexponential factors. The activation energy of R_{1} exceeds R_{2} by $10{\mathrm{kJmol}}^{1}$.k_{1} and k_{2} are two rate constants for reaction R_{1} and R_{2} at$300\mathrm{K}$, then the ratio of $\frac{{\mathrm{k}}_{2}}{{\mathrm{k}}_{1}}$ will be?( R=$8.314{\mathrm{Jmol}}^{1}{\mathrm{K}}^{1}$)
$6$
$4$
$8$
$12$
Distinguish between specific reaction rate and rate of the reaction
The rate of a chemical reaction doubles for every $10\xb0\mathrm{C}$ rise in temperature. If the temperature is raised by $50\xb0\mathrm{C}$, The rate of the reaction increases by about?
For the decomposition of azoisopropane to hexane and nitrogen at 543 K, the following data are obtained. Calculate the rate constant.
t(s)p(mm of Hg)035.036054.072063.0
 2.303 Mmin−1
 0.2303 Mmin−1
 0.1 Mmin−1
 None of these
(Given : log 2 = 0.3010, log 4 = 0.6021, R = 8.314 JK−1 mol−1)
${\mathbf{NaClO}}_{\mathbf{3}}$ is used, even in spacecrafts, to produce ${\mathbf{O}}_{\mathbf{2}}$. The daily consumption of pure ${\mathbf{O}}_{\mathbf{2}}$ by a person is 492 L at 1 atm, 300 K. How much amount of ${\mathbf{NaClO}}_{\mathbf{3}}$, in grams, is required to produce ${\mathbf{O}}_{\mathbf{2}}$ for the daily consumption of a person at 1 atm, 300 K?
${\mathrm{NaClO}}_{3}\left(\mathrm{s}\right)+\mathrm{Fe}\left(\mathrm{s}\right)\to {\mathrm{O}}_{2}\left(\mathrm{g}\right)+\mathrm{FeO}\left(\mathrm{s}\right)+\mathrm{NaCl}\left(\mathrm{s}\right)\phantom{\rule{0ex}{0ex}}\mathrm{R}=0.082\mathrm{L}\mathrm{atm}{\mathrm{mol}}^{\u20131}{\mathrm{K}}^{\u20131}$
 A = 50 atm, B = 100 atm
 A = 100 atm, B = 200 atm
 A = 50 atm, B = 30 atm
 A = 50 atm, B = 200 atm
(log 2 = 0.3)
 50 min
 20 min
 150 min
 100 min
 0.0693 mole Lmin−1
 0.0693×2.5 mol L−1 min−1
 0.693×5 mol L−1 min−1
 0.693×10 mol L−1min−1
 4.60×10−3s−1
 4.90×10−3s−1
 1.15×10−3s−1
 6.9×10−2s−1
Initial concentration (A)  Initial concentration (B)  Initial rate of formation of C (molL1S−1) 
0.1M  0.1M  1.2×10−3 
0.1M  0.2M  1.2×10−3 
0.2M  0.1M  2.4×10−3 
The rate law for the formation of C is :
(IITJEE2014)
dcdt=k[A]
 dcdt=k[A][B]
 dcdt=k[A]2[B]
dcdt=k[A][B]2
The rate constant ${k}_{1}$ of a reaction is found to be double that of rate constant ${k}_{2}$ of another reaction. The relationship between corresponding activation energies of the two reactions at the same temperature (${E}_{1}$ and ${E}_{2}$) can be represented as:
(Given log2=0.3010)
 10 min
 20 min
 30 min
 40 min
 10−4s−1
 6×10−2s−1
 10−2s−1
 6×102s−1