Which of the following rate laws has an over all order of 0.5 for the reaction A+B+C$\to$product-

(1) R= k [A][B][C]                                    

(2) $R=k\left[A{]}^{0.5}\right[B{]}^{0.5}[C{]}^{0.5}$

(3) $R=k\left[A{]}^{1.5}\right[B{]}^{-1}[C{]}^0$                                

(4) $R=k\left[A\right] \left[B{]}^0\right[C{]}^{0.5}$

For a reaction of the type 2A + B $\to$ 2C, the rate of the reaction is given by $k{\left[A\right]}^2\left[B\right]$. When the volume of the reaction vessel is reduced to $\frac{1}{4}$ th of the original volume, the rate of reaction changes by a factor of:

1. 0.25                                                          

2. 16

3. 64                                                             

4. 4

The rate constant of a first order reaction is generally determined from a plot of 

(1) Concentration of reactant vs time t

(2) log (concentration of reactant) vs time t

(3) $\frac{1}{concentration of reac\tan t} vs time t$

(4) Concentration of reactant vs log time t

The plot of log k versus \(1 \over T\) is linear with a slope of:

The rate constant , the activation energy and the Arrhenius parameter of a chemical reaction at 25°C are $3.0 \times {10}^{-4} s^{-1}$ $,104.4 kJ mo{l}^{-4}$and $6.0 \times {10}^{-14}$ s–1 respectively the value of the rate constant as T$\to \infty$ is :

(1) $2.0\times {10}^{18} s^{-1}$                                                  

(2) $6.0\times {10}^{-14}{s}^{-1}$

(3) $\infty$                                                                   

(4) $3.6\times {10}^{30} s^{-1}$

87.5% of a radioactive substance disintegrates in 40 minutes. What is the half life of the substance ?

(1) 13.58 min                                                   

(2) 135.8 min

(3) 1358 min                                                    

(4) None of these

If 60 % of a first-order reaction is completed in 60 minutes, 50 % of the same reaction takes approximately:
(log4 = 0.60, log5 = 0.69)

For the reaction, N₂ + 3H₂ $\to$2NH₃, if $\frac{\mathrm{d}\left[{\mathrm{NH}}_3\right]}{\mathrm{dt}}$= 2x10^-4 mol L^-1s^-1, the value of $-\frac{\mathrm{d}\left[{\mathrm{H}}_2\right]}{\mathrm{dt}}$ would be :

1. 3x10^-4 mol L^-1s^-1

2. 4x10^-4 mol L^-1s^-1

3. 6x10^-4 mol L^-1s^-1

4. 1x10^-4 mol L^-1s^-1

Half-life period of a first order reaction is 1386s. The specific rate constant of the reaction is

(a) 5.0 x 10^-3s^-1

(b) 0.5 x 10^-2s^-1

(c) 0.5 x 10^-3s^-1

(d) 5.0 x 10^-2s^-1

Which one of the following statements for the order of a reaction is incorrect?

(1) Order is not influenced by stiochiometric coefficient of the reactants

(2) Order of reaction is sum of power to the concentration terms of reactants to express the rate of reaction

(3) Order of reaction is always whole number

(4) Order can be determined only experimentally