Question 1 :
The sum of the powers of the concentration terms that occur in the rate equation is called:
Question 3 : 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 4 :
For which of the following, the units of rate and rate constant of the reaction is identical?
Question 6 :
A zero order reaction is one in which the rate of the reaction is independent of ______________.<br/>
Question 7 :
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 9 :
The time required for $100\%$ completion of a zero order reaction is:
Question 10 : The rate law for the reaction<div><br/>RCl + NaOH $\rightarrow$ 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 reaction<br/>iv) is unaffected by change in temperature<br/>The correct combination is:<br/></div>
Question 11 :
The reaction between $NO$ and ${ Cl }_{ 2 }$ takes place in the following two steps:<br/>$I$. $NO+{ Cl }_{ 2 }\overset {{ k }_{ 1 } }{ \underset { \underset { fast }{ { k }_{ 2 } }  }{ \rightleftharpoons  }  } NO{ Cl }_{ 2 }$<br/>$II$. $NO{ Cl }_{ 2 }+NO\xrightarrow [ slow ]{ \quad { k }_{ 3 }\quad  } 2NOCl$<br/>The rate law of overall reaction, $2NO+{ Cl }_{ 2 }\longrightarrow 2NOCl$, can be given by:
Question 12 :
The rate equation for the reaction $ 2A+B\rightarrow C$ is found to be : $rate=k[A] [B].$ The correct statement in relation to this reaction is:
Question 13 : For a reaction, $I^{-} + OCl^{-} \rightarrow IO^{-} + Cl^{-}$ in an aqueous medium, the rate of reaction is given by<br/><div> $\dfrac {d[IO^{-}]}{dt} = k \dfrac {[I^{-}][OCl^{-}]}{[OH^{-}]}$. The overall order of reaction is ?</div>
Question 14 :
Assertion: The order of a reaction can have fractional value.
Reason: The order of a reaction cannot be written from balanced equation of a reaction.
Question 15 :
The rate constant of a reaction is found to be $3\times { 10 }^{ -3 }$ $mol$ ${ L }^{ -1 }$ ${ min }^{ -1 }$. The order of the reaction is:
Question 16 :
In a given reaction under standard conditions in a closed container, which type of reaction would show no real increase in the rate of the reaction when the concentration of each reactant is doubled?
Question 17 :
If the concentration of the reactants in the reaction $\:2A+B\rightarrow C+D\:$ is increased by three folds, the rate of the reaction will be increased by:
Question 18 :
If 'a' is the initial concentration of a substance which reacts according to zero order kinetics and K is rate constant, the time for the reaction to go to completion is:<br/>
Question 19 : The following are the data for the reaction <div><br/></div><div>      $A+B\rightarrow $ products </div><div><br/></div><div>        [A]               [B]            Initial rate $(mol\, L^{-1}s^{-1})$<br/>(i)    0.1 M        0.1 M                  $4.0\times 10^{-4}$<br/>(ii)   0.2 M        0.2 M                  $1.6\times 10^{-3}$<br/>(iii)  0.5 M        0.1 M                  $1.0\times 10^{-2}$<br/>(iv)  0.5 M        0.5 M                  $1.0\times 10^{-2}$ <div><br/><div>The rate constant of the reaction is _________ .<br/><br/></div></div></div>
Question 20 :
For a reaction $P \rightarrow Q$, the half-life of the reaction was 3h, when the initial concentration of P was 0.5M. As the concentration of P was increased to 1.0M, half life changes to 6h. The order of reaction with respect to P is:
Question 21 :
In which of the following reactions of the following orders the molecularity and order can never be same?
Question 22 :
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:
Question 23 :
Activation energy $(E_a)$ and rate constants ($k_1$ and $k_2$) of a chemical reaction at two different temperature ($T_1$ and $T_2$) are related by:
Question 24 :
In a reaction, the concentration of reactant is increased two times and three times then the increases in rate of reaction were four times and nine times respectively, order of reaction is:
Question 25 :
Assertion: Molecularity has no meaning for a complex reaction.
Reason: The overall molecularity of a complex reaction is equal to the molecularity of the slowest step.
Question 26 :
The rate of a certain reaction is given by, rate $=k{ \left[ { H }^{ + } \right]  }^{ n }$. The rate increases 100 times when the pH changes from 3 to 1. The order $\left( n \right) $ of the reaction is:
Question 27 :
For a homogeneous gaseous reaction $A \rightarrow 3B,$ if pressure after time t was $P_{r}$ and after completion of reaction, pressure was $P_{\infty}$ then select correct relation
Question 30 :
The order of a reaction is said to be $2$ with respect to a reactant $X$ when:
