Question 1 :
The order and molecularity of the chain reaction, ${ H }_{ 2 }\left( g \right) +{ Cl }_{ 2 }\left( g \right) \xrightarrow [  ]{  \quad hv\quad  } 2HCl\left( g \right) $, are:

Question 2 :
The sum of the powers of the concentration terms that occur in the rate equation is called:

Question 5 :
A zero order reaction is one in which the&#160;rate of the reaction&#160;is&#160;independent of ______________.<br/>

Question 6 :
For which of the following, the units of rate and rate constant of the reaction is identical?

Question 7 :
From the following data estimate the order for decomposition of an aqueous solution of hydrogen peroxide:<table class="wysiwyg-table"><tbody><tr><td>Time (minutes)</td><td>$0$</td><td>$10$</td><td>$20$</td><td>$30$</td></tr><tr><td>$V(ml)$</td><td>$46.1$</td><td>$29.8$</td><td>$19.6$</td><td>$12.3$</td></tr></tbody></table>where $V$ is the volume of potassium permanganate solution in $mL$ required to decompose a definite volume of the peroxide solution.

Question 10 :
The rate constant of a reaction is equal to rate of reaction:

Question 12 :
Which one of the following statements for order of a reaction is not correct?

Question 13 :
For reaction; $A\rightarrow B$, the rate of constant ${ k }_{ 1 }={ A }_{ 1 }{ e }^{ -E{ a }_{ 1 }/RT }$ and for the reaction; $P\rightarrow Q\quad $, the rate constant ${ k }_{ 2 }={ A }_{ 2 }{ e }^{ -E{ a }_{ 2 }/RT }$. If ${ A }_{ 1 }={ 10 }^{ 8 },{ A }_{ 2 }={ 10 }^{ 10 }$ and $E{ a }_{ 1 }=600,E{ a }_{ 2 }=1200$, then the temperature at which ${ k }_{ 1 }={ k }_{ 2 }$ is:

Question 14 :
A reaction is second order with respect to a reactant. If the concentration of reactant is doubled&#160;the rate of reaction becomes :

Question 15 :
The rate law for the reaction<div><br/>RCl + NaOH $\rightarrow$&#160;ROH + NaCl is given by<br/>r $=$ k[RCl] the rate of reaction is</div><div><br/>i) double by doubling the conc. of NaOH<br/>ii) is halved by reducing conc. of RCl by one half<br/>iii) is increased by increasing the temperature of&#160;reaction<br/>iv) is unaffected by change in temperature<br/>The correct combination is:<br/></div>

Question 16 :
Substance A reacts according to a first order rate law with&#160;$k\,=\,5.0\times10^{-5}\,s^{-1}.$ If the initial conc. of A is $1.0\;M,$ the initial rate is:

Question 17 :
For the reaction, $2NO\longrightarrow { N }_{ 2 }+{ O }_{ 2 }$, the expression $-\dfrac { 1 }{ 2 } \dfrac { d\left[ NO \right] &#160;}{ dt } $ represents:

Question 18 :
In a reaction A+B $\rightarrow $ products, the rate of reaction&#160;is doubled when the concentration of A is doubled&#160;and B is kept constant and the rate of the reaction&#160;is increased by 8 times when the concentrations&#160;of both A and B are doubled, thus overall order of&#160;the reaction is:<br/>

Question 19 :
The relation between the rate of a simple reaction&#160;and the concentration '$c$' of a&#160;reacting species is given as:<br/>

Question 20 :
For a reaction that has $[A]$ and $[B]$ both doubled, the rate goes up by a factor of $8$. The rate law is: $rate = k[A]^{m}[B]^{2}$.<br>What is the rate order with respect to $[A]$?

Question 21 :
If $50$% of a reaction occurs in 100 second and $75$% of the reactions occurs in 200 seconds, the order of this reaction is ?

Question 22 :
For the reaction, $H_{2}(g) + Br_{2}(g)\rightarrow 2HBr(g)$, then reaction $rate = K\ [H_{2}]\,[Br_{2}]^{1/2}$. Which statement is true about this reaction :

Question 23 :
Assertion: Complex reaction takes place in different step and the slowest step determines the rate of reaction. Reason: Order and molecularity of a reaction are always equal.

Question 24 :
In a zero order reaction half life is 100 sec. After how much time 78 fraction of reactant will be reacted?

Question 25 :
For a certain reaction the expression for half life is&#160; $t \propto \frac{1}{{{a^{n - 1}}}}$ then the order of reaction is:

Question 26 :
The concentration of a reactant in a solution falls from 0.2 M to 0.1 M in 2 hours and to 0.05 M in 4 hours. The order of reaction is:

Question 28 :
Two gases A and B are filled in a container. The experimental rate law for the reaction between them is $Rate = k [A]^2[B]$. Predict the effect on the rate of the reaction when pressure is doubled: