For the reaction $R-X+OH \to ROH+$$X^{-}$ The rate is given of

Rate=$5.0\times {10}^{-5}\left[R-X\right]\left[O{H}^{-}\right]+0.20\times {10}^{-5}\left[R-X\right]$ what percentage of R-X Reaction by $S{N}^2$ mechanism when $\left[O{H}^{-}\right]=1.0\times {10}^{-2}M$

The curve that  represents a 1st order reaction is: 

The rate of a reaction increases 4-fold when when concentration of reactant is incresed 16 times. If the rate of reaction is $4\times {10}^{-6} mole L^{-1}{s}^{-1}$when concentration of the reactant is $4\times {10}^{-4}$ $\mathrm{mol} {\mathrm{L}}^{-1}$, the rate constant of the reaction will be : 

If ‘a’ is the initial concentration of a substance which reacts according to zero order kinetic and k is rate constant, the time for the reaction to go to completion is-

The following data are obtained from the decomposition of a gaseous compound -

Initial pressure, atm               1.6       0.8       0.4

Time for 50% reaction, min     80       113      160

The order of the reaction is : 

For a given reaction the concentration of the reactant plotted against time gave a straight line with negative slope.

The order of the reaction is-

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

The correct representation of  the variation of the rate of the reaction with temperature is: 

The plot of log k versus $\frac{1}{T}$ is linear with a slope of

If a reaction A + B$\to$ C is exothermic to the extent of 30 kJ/mol and the forward reaction has an activation energy 70 kJ/mol, the activation energy for the reverse reaction is :

For a certain reaction involving a single reactant, it is found that $C_0\sqrt{T}$ is constant where $C_0$is the initial concentration of the reactant and T is the half-life. What is the order of the reaction ?

The high temperature ($\approx$ 1200K) decomposition of $C{H}_{3}COOH$(g) occurs as follows as per simultaneous 1st order reactions.

$C{H}_{3}COOH \stackrel{k_1}{\to } C{H}_4+ C{O}_2$

$C{H}_{3}COOH \stackrel{k_2}{\to } C{H}_{2}CO + H_{2}O$

What would be the % of $C{H}_4$by mole in the product mixture (excluding$C{H}_{3}COOH$)?

The reaction , A(g) + 2B(g) C(g) + D(g) is an elementary process. In an experiment, the initial partial pressure of A and B are $P_A$= 0.60 and $P_B$= 0.80 atm. When $P_C$= 0.2atm the rate of reaction relative to the initial rate is

Half life period for a first order reaction is 20 minutes. Time required to change the concentration of the reactants from 0.08 M to 0.01M is: 

The kinetic data for the reaction: 2A + B₂$\to$2AB are as given below:

$$\begin{gathered} \left[\mathrm{A}\right] \left[{\mathrm{B}}_2\right] \mathrm{Rate} \\ \mathrm{mol} {\mathrm{L}}^{-1 } \mathrm{mol} {\mathrm{L}}^{-1} \mathrm{mol} {\mathrm{L}}^{-1}{\mathrm{s}}^{-1} \\ 0.5 1.0 2.5\times {10}^{-3} \\ 1.0 1.0 5.0\times {10}^{-3} \\ 0.5 2.0 1\times {10}^{-2} \end{gathered}$$

The order of reaction w.r.t. A and $B_2$ are respectively :

1. 1 and 2

2. 2 and 1

For the irreversible unimolecular type reaction A $\stackrel{k}{\to }$products in a batch reactor, 80% reactant A($C_{A0} = 1 mole/lit.)$is converted in a 480 second run and conversion is 90% after 18 minute. The order of this reaction is-

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

The gas phase decomposition $2N_2{O}_5\to 4N{O}_2+ O_2$ follows the first order rate law.$K = 7.5 \times {10}^{-3}$$se{c}^{-1}$. The initial pressure of $N_2{O}_5$is 0.1 atm. The time of decomposition of $N_2{O}_5$ so that the total pressure becomes 0.15 atm will be-

If in the fermentation of sugar in an enzymatic solution that is 0.12 M, the concentration of the sugar is reduced to 0.06 M in 10h and to 0.03 M in 20h, the order of the reaction is:

In a first order reaction A $\to$ products, the concentration of the reactant decreases to 6.25% of its initial value in 80 minutes. The value of the rate constant, if the initial concentration is 0.2 mole/litre will be :

A catalyst lowers the activation energy of a reaction from 20 kJ $mol{e}^{–1}$ to 10 kJ $mol{e}^{–1}$. The temperature at which the uncatalysed reaction will have the same rate as that of the catalysed at $27°C$is :

For a certain reaction the variation of the rate constant with temperature is given by the equation

                            $In k_1=In k_0+\left(\frac{In 3}{10}\right)t \left(t\ge 0°C\right)$

The value of the temperature coefficient of the reaction rate is therefore –

A catalyst lowers the activation energy of a reaction from $20 kJ mol{e}^{-1} to 10 kJ mol{e}^{-1}$. The temperature at which the uncatalysed reaction will have the same rate as that of the catalysed at $27°C$ is :

The rate of reaction triples when temperature change from $20°\mathrm{C} \mathrm{to} 50°\mathrm{C}$. The energy of activation for the reaction is- 

The half-life time for the decomposition of a substance dissolved in ${\mathrm{CCl}}_4$ is 2.5 hour at $30°$C. The amount of substance that will  left after 10 hours if the initial weight of the substance is 160 gm is: 

If the values of the rate constants are $3.45\times {10}^{-5 }and 6.9\times {10}^{-3} at 27°C and 67°C$ respectively. The activation energy for the decomposition of $N_2{O}_5 as N_2{O}_5 \rightleftharpoons 2N{O}_2+ (1/2) O_2$ is: 

The percentage of the reactant molecules crossing over the energy barrier at 325 K is: 

Given that $∆{\mathrm{H}}_{325}=0.12 \mathrm{kcal}, {\mathrm{E}}_{\mathrm{a}\left(\mathrm{b}\right)}=+0.02 \mathrm{kcal}$

1 mole of gas changes linearly from initial state (2 atm, 10 lt) to final state (8 atm, 4 lt). Maximum rate constant is equal to 20 $se{c}^{-1}$ and value of activation energy is 40 kJ $mol{e}^{-1}$, assuming that activation energy does not change in this temperature range.The value of rate constant, at the maximum temperature, that the gas can attain is: 

A first order reaction was started with a decimolar solution of the reactant. After 8 minutes and 20 seconds, its concentration was found to be M/100. The rate constant of the reaction is: 

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