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MCQOPTIONS
This section includes 11242 Mcqs, each offering curated multiple-choice questions to sharpen your Joint Entrance Exam - Main (JEE Main) knowledge and support exam preparation. Choose a topic below to get started.
| 1151. |
When the concentration of A in the reaction \[A+B\]⇌\[AB\] is doubled, the rate of reaction will be [MP PMT 2002] |
| A. | Doubled |
| B. | Decreased by half |
| C. | Unchanged |
| D. | Increased by four times |
| Answer» B. Decreased by half | |
| 1152. |
The rate of a chemical reaction depends upon [AFMC 2002] |
| A. | Time |
| B. | Pressure |
| C. | Concentration |
| D. | All of these |
| Answer» E. | |
| 1153. |
For the reaction \[{{N}_{2}}+3{{H}_{2}}\to 2N{{H}_{3}}\] if \[\frac{\Delta [N{{H}_{3}}]}{\Delta t}=2\times {{10}^{-4}}mol\,{{l}^{-1}}{{s}^{-1}},\] the value of \[\frac{-\Delta [{{H}_{2}}]}{\Delta t}\] would be [MP PMT 2000] |
| A. | \[1\times {{10}^{-4}}mol\,\,{{l}^{-1}}{{s}^{-1}}\] |
| B. | \[3\times {{10}^{-4}}mol\,\,{{l}^{-1}}{{s}^{-1}}\] |
| C. | \[4\times {{10}^{-4}}mol\,\,{{l}^{-1}}{{s}^{-1}}\] |
| D. | \[6\times {{10}^{-4}}mol\,{{l}^{-1}}{{s}^{-1}}\] |
| Answer» C. \[4\times {{10}^{-4}}mol\,\,{{l}^{-1}}{{s}^{-1}}\] | |
| 1154. |
For a given reaction \[3A+B\to C+D\] the rate of reaction can be represented by [DCE 2000] |
| A. | \[-\frac{1}{3}\frac{d[A]}{dt}=\frac{-d[B]}{dt}=\frac{+d[C]}{dt}=\frac{+d[D]}{dt}\] |
| B. | \[-\frac{1}{3}\frac{d[A]}{dt}=\frac{d[C]}{dt}=K{{[A]}^{m}}{{[B]}^{n}}\] |
| C. | \[+\frac{1}{3}\frac{d[A]}{dt}=\frac{-d[C]}{dt}=K{{[A]}^{n}}{{[B]}^{m}}\] |
| D. | None of these |
| Answer» B. \[-\frac{1}{3}\frac{d[A]}{dt}=\frac{d[C]}{dt}=K{{[A]}^{m}}{{[B]}^{n}}\] | |
| 1155. |
The rate of a reaction that not involve gases is not dependent on [CPMT 1988; AFMC 1995] |
| A. | Pressure |
| B. | Temperature |
| C. | Concentration |
| D. | Catalyst |
| Answer» B. Temperature | |
| 1156. |
The rate of a reaction depends upon the [Pb. PMT 1999] |
| A. | Volume |
| B. | Force |
| C. | Pressure |
| D. | Concentration of reactant |
| Answer» E. | |
| 1157. |
The term \[\left( -\frac{dc}{dt} \right)\] in a rate equation refers to the [MP PMT 1996] |
| A. | Concentration of the reactant |
| B. | Decrease in concentration of the reactant with time |
| C. | Increase in concentration of the reactant with time |
| D. | Velocity constant of the reaction |
| Answer» C. Increase in concentration of the reactant with time | |
| 1158. |
In the reaction \[2A+B\to {{A}_{2}}B\], if the concentration of \[A\] is doubled and of \[B\] is halved, then the rate of the reaction will [MP PET 1994; CBSE PMT 2000] |
| A. | Increase by four times |
| B. | Decrease by two times |
| C. | Increase by two times |
| D. | Remain the same |
| Answer» D. Remain the same | |
| 1159. |
For the reaction \[{{N}_{2}}(g)+3{{H}_{2}}(g)\to 2N{{H}_{3}}(g)\] under certain conditions of temperature and partial pressure of the reactants, the rate of formation of \[N{{H}_{3}}\] is \[0.001\,kg\,{{h}^{-1}}\]. The rate of conversion of \[{{H}_{2}}\] under the same conditions is [IIT 1994] |
| A. | \[1.82\,\times {{10}^{-4}}\,kg/hr\] |
| B. | \[0.0015\,kg/hr\] |
| C. | \[1.52\times {{10}^{4}}kg/hr\] |
| D. | \[1.82\times {{10}^{-14}}kg/hr\] |
| Answer» C. \[1.52\times {{10}^{4}}kg/hr\] | |
| 1160. |
A catalyst increases the rate of reaction because it [EAMCET 1992] |
| A. | Increases the activation energy |
| B. | Decreases the energy barrier for reaction |
| C. | Decreases the collision diameter |
| D. | Increases the temperature coefficient |
| Answer» C. Decreases the collision diameter | |
| 1161. |
In a reaction \[2A+B\to {{A}_{2}}B\], the reactant A will disappear at [MP PET 1993] |
| A. | Half the rate that B will decrease |
| B. | The same rate that B will decrease |
| C. | Twice the rate that B will decrease |
| D. | The same rate that \[{{A}_{2}}B\] will form |
| Answer» D. The same rate that \[{{A}_{2}}B\] will form | |
| 1162. |
For reaction \[2A+B\to \] products, the active mass of B is kept constant and that of A is doubled. The rate of reaction will then [MP PET 1993] |
| A. | Increase 2 times |
| B. | Increase 4 times |
| C. | Decrease 2 times |
| D. | Decrease 4 times |
| Answer» C. Decrease 2 times | |
| 1163. |
Time required for completion of ionic reactions in comparison to molecular reactions is |
| A. | Maximum |
| B. | Minimum |
| C. | Equal |
| D. | None |
| Answer» C. Equal | |
| 1164. |
If the concentration of the reactants is increased, the rate of reaction [MP PMT 1989] |
| A. | Remains unaffected |
| B. | Increases |
| C. | Decreases |
| D. | May increase or decrease |
| Answer» C. Decreases | |
| 1165. |
The rate of a chemical reaction [MP PMT 1973; CPMT 1982] |
| A. | Increases as the reaction proceeds |
| B. | Decreases as the reaction proceeds |
| C. | May increase or decrease during the reaction |
| D. | Remains constant as the reaction proceeds |
| Answer» C. May increase or decrease during the reaction | |
| 1166. |
The order of a reaction with rate equals \[kC_{A}^{3/2}\,C_{B}^{-1/2}\] is [MP PET 1996, 2001] |
| A. | 2 |
| B. | 1 |
| C. | \[-\frac{1}{2}\] |
| D. | \[\frac{3}{2}\] |
| Answer» C. \[-\frac{1}{2}\] | |
| 1167. |
If the rate expression for a chemical reaction is given by Rate \[=k{{[A]}^{m}}{{[B]}^{n}}\] [MP PMT 1996] |
| A. | The order of the reaction is \[m\] |
| B. | The order of the reaction is \[n\] |
| C. | The order of the reaction is \[m+n\] |
| D. | The order of the reaction is \[m-n\] |
| Answer» D. The order of the reaction is \[m-n\] | |
| 1168. |
The half-life period of a first order reaction is 100 sec. The rate constant of the reaction is [MP PMT 1997; MP PET 2001] |
| A. | \[6.93\times {{10}^{-3}}{{\sec }^{-1}}\] |
| B. | \[6.93\times {{10}^{-4}}{{\sec }^{-1}}\] |
| C. | \[0.693\,{{\sec }^{-1}}\] |
| D. | \[69.3\,{{\sec }^{-1}}\] |
| Answer» B. \[6.93\times {{10}^{-4}}{{\sec }^{-1}}\] | |
| 1169. |
In a reaction involving hydrolysis of an organic chloride in presence of large excess of water \[RCl+{{H}_{2}}O\to ROH+HCl\] [MP PET 1995] |
| A. | Molecularity is 2, order of reaction is also 2 |
| B. | Molecularity is 2, order of reaction is 1 |
| C. | Molecularity is 1, order of reaction is 2 |
| D. | Molecularity is 1, order of reaction is also 1 |
| Answer» C. Molecularity is 1, order of reaction is 2 | |
| 1170. |
The reaction \[2{{H}_{2}}{{O}_{2}}\to 2{{H}_{2}}O+{{O}_{2}}\] is a [Manipal MEE 1995] |
| A. | Zero order reaction |
| B. | First order reaction |
| C. | Second order reaction |
| D. | Third order reaction |
| Answer» C. Second order reaction | |
| 1171. |
Half life period of second order reaction is [MP PMT 1994] |
| A. | Proportional to the initial concentration of reactants |
| B. | Independent of the initial concentration of reactants |
| C. | Inversely proportional to initial concentration of reactants |
| D. | Inversely proportional to square of initial concentration of reactants |
| Answer» D. Inversely proportional to square of initial concentration of reactants | |
| 1172. |
The half life of a first order reaction is 10 minutes. If initial amount is \[0.08\,mol/litre\] and concentration at some instant is \[0.01\,mol/litre\], then \[t=\] [Roorkee 1990] |
| A. | 10 minutes |
| B. | 30 minutes |
| C. | 20 minutes |
| D. | 40 minutes |
| Answer» C. 20 minutes | |
| 1173. |
The half life of a first order reaction is \[69.35\,\sec \]. The value of the rate constant of the reaction is [CBSE PMT 1990] |
| A. | \[1.0\,{{s}^{-1}}\] |
| B. | \[0.1\,{{s}^{-1}}\] |
| C. | \[0.01\,{{s}^{-1}}\] |
| D. | \[0.001\,{{s}^{-1}}\] |
| Answer» D. \[0.001\,{{s}^{-1}}\] | |
| 1174. |
Diazonium salt decomposes as \[{{C}_{6}}{{H}_{5}}N_{2}^{+}C{{l}^{-}}\to {{C}_{6}}{{H}_{5}}Cl+{{N}_{2}}\] At \[{{0}^{o}}C\], the evolution of \[{{N}_{2}}\] becomes two times faster when the initial concentration of the salt is doubled. Therefore, it is [MNR 1994; UPSEAT 2002] |
| A. | A first order reaction |
| B. | A second order reaction |
| C. | Independent of the initial concentration of the salt |
| D. | A zero order reaction |
| Answer» B. A second order reaction | |
| 1175. |
In the reaction \[A+B\to \] Products, if \[B\] is taken in excess, then it is an example of [EAMCET 1992] |
| A. | Second order reaction |
| B. | Zero order reaction |
| C. | Pseudounimolecular reaction |
| D. | First order reaction |
| Answer» D. First order reaction | |
| 1176. |
For a reaction \[2A+B\to \]Products, doubling the initial concentration of both the reactants increases the rate by a factor of 8, and doubling the concentration of B alone doubles the rate. The rate law for the reaction is [MP PET 2001] |
| A. | \[\gamma =k[A]{{[B]}^{2}}\] |
| B. | \[\gamma =k{{[A]}^{2}}[B]\] |
| C. | \[\gamma =k[A][B]\] |
| D. | \[\gamma =k{{[A]}^{2}}{{[B]}^{2}}\] |
| Answer» C. \[\gamma =k[A][B]\] | |
| 1177. |
The incorrect order indicated against the rate of reaction \[A+B\xrightarrow{K}C\] is [BHU 1990] |
| A. | Rate Order \[\frac{d[C]}{dt}=K[A]\] 1 |
| B. | \[\frac{d[C]}{dt}=K[A]\,[B]\] 2 |
| C. | \[\frac{-d\,[A]}{dt}=K\,[A]\,{{[B]}^{0}}\] 2 |
| D. | \[\frac{-d\,[A]}{dt}\,K\,[A]\] 1 |
| Answer» D. \[\frac{-d\,[A]}{dt}\,K\,[A]\] 1 | |
| 1178. |
Which of the following statements regarding the molecularity of a reaction is wrong [CBSE PMT 1989] |
| A. | It is the number of molecules of the reactants taking part in a single step chemical reaction |
| B. | It is calculated from the reaction mechanism |
| C. | It may be either a whole number or fractional |
| D. | It depends on the rate determining step in the reaction |
| Answer» D. It depends on the rate determining step in the reaction | |
| 1179. |
The unit of the velocity constant in case of zero order reaction is [CPMT 1994] |
| A. | \[Conc.\times tim{{e}^{-1}}\] |
| B. | \[Conc{{.}^{-1}}\times time\] |
| C. | \[Conc{{.}^{-1}}\times tim{{e}^{-1}}\] |
| D. | \[Conc.\times {{(time)}^{2}}\] |
| Answer» B. \[Conc{{.}^{-1}}\times time\] | |
| 1180. |
For the reaction \[{{H}_{2}}(g)+B{{r}_{2}}(g)\to 2HBr(g)\], the experimental data suggest, rate \[=K[{{H}_{2}}]{{[B{{r}_{2}}]}^{1/2}}\]. The molecularity and order of the reaction are respectively [CPMT 1988; MP PET 1993] |
| A. | \[2,\,\frac{3}{2}\] |
| B. | \[\frac{3}{2},\,\frac{3}{2}\] |
| C. | 1, 1 |
| D. | \[1,\,\frac{1}{2}\] |
| Answer» B. \[\frac{3}{2},\,\frac{3}{2}\] | |
| 1181. |
For any reaction, if we plot a graph between time ?t? and \[\log (a-x)\], a simple line is obtained. The order of reaction is |
| A. | Zero |
| B. | One |
| C. | Two |
| D. | Three |
| Answer» C. Two | |
| 1182. |
Molecularity of reaction of inversion of sugar is |
| A. | 3 |
| B. | 2 |
| C. | 1 |
| D. | 0 |
| Answer» C. 1 | |
| 1183. |
If the surface area of the reactants increases, then order of the reaction |
| A. | Increases |
| B. | Decreases |
| C. | Remain constant |
| D. | Sometimes increases and sometimes dereases |
| Answer» D. Sometimes increases and sometimes dereases | |
| 1184. |
Half life period \[{{t}_{1/2}}\] for first order reaction is |
| A. | K |
| B. | \[\frac{1.303\,\log \,2}{K}\] |
| C. | \[\frac{2.303\,\log \,2}{K}\] |
| D. | \[\frac{9}{K}\] |
| Answer» D. \[\frac{9}{K}\] | |
| 1185. |
The reaction \[2NO(g)+{{O}_{2}}(g)\]⇌\[2N{{O}_{2}}(g)\]is of first order. If volume of reaction vessel is reduced to 1/3, the rate of reaction would be [MP PMT 2001] |
| A. | 1/3 times |
| B. | 2/3 times |
| C. | 3 times |
| D. | 6 times |
| Answer» D. 6 times | |
| 1186. |
The one which is unimolecular reaction is [MP PMT 1999; UPSEAT 2001] |
| A. | \[2HI\to {{H}_{2}}+{{I}_{2}}\] |
| B. | \[{{N}_{2}}{{O}_{5}}\to {{N}_{2}}{{O}_{4}}+\frac{1}{2}{{O}_{2}}\] |
| C. | \[{{H}_{2}}+C{{l}_{2}}\to 2HCl\] |
| D. | \[PC{{l}_{3}}+C{{l}_{2}}\to PC{{l}_{5}}\] |
| Answer» C. \[{{H}_{2}}+C{{l}_{2}}\to 2HCl\] | |
| 1187. |
Integrated velocity equation for first order reaction is |
| A. | \[{{[A]}_{o}}=[A]\,{{e}^{-Kt}}\] |
| B. | \[K={{[A]}_{o}}{{e}^{-A/t}}\] |
| C. | \[Kt=2.303\,\log \,\frac{{{[A]}_{o}}}{[A]}\] |
| D. | \[\log \,\frac{{{[A]}_{o}}}{[A]}=-2.303\,Kt\] |
| Answer» D. \[\log \,\frac{{{[A]}_{o}}}{[A]}=-2.303\,Kt\] | |
| 1188. |
Inversion of sucrose is [AMU 1988; MP PET 2000] |
| A. | Zero order reaction |
| B. | First order reaction |
| C. | Second order reaction |
| D. | Third order reaction |
| Answer» C. Second order reaction | |
| 1189. |
The alkaline hydrolysis of ethyl acetate is represented by the equation \[C{{H}_{3}}COO{{C}_{2}}{{H}_{5}}+NaOH\to C{{H}_{3}}COONa+{{C}_{2}}{{H}_{5}}OH\] Experimentally it is found that for this reaction \[\frac{dx}{dt}=k[C{{H}_{3}}COO{{C}_{2}}{{H}_{5}}]\,[NaOH]\] Then the reaction is [JIPMER 1999] |
| A. | Bimolecular and of first order |
| B. | Bimolecular and of second order |
| C. | Pseudo?bimolecular |
| D. | Pseudo?unimolecular |
| Answer» C. Pseudo?bimolecular | |
| 1190. |
A reaction \[2A\to \] products is found to follow zero oder kinetics, then |
| A. | \[\frac{dx}{dt}=k{{[A]}^{2}}\] |
| B. | \[\frac{dx}{dt}=k{{[A]}^{0}}\] |
| C. | \[\frac{dx}{dt}=k[A]\] |
| D. | \[\frac{dx}{dt}=k[2A]\] |
| Answer» C. \[\frac{dx}{dt}=k[A]\] | |
| 1191. |
Decomposition of nitrogen pentoxide is known to be a first order reaction 75 percent of the oxide had decomposed in the first 24 minutes. At the end of an hour, after the start of the reaction, the amount of oxide left will be |
| A. | Nil |
| B. | About 1% |
| C. | About 2% |
| D. | About 3% |
| Answer» E. | |
| 1192. |
About half life period of a first order reaction, which one of the following statements is generally false |
| A. | It is independent of initial concentration |
| B. | It is independent of temperature |
| C. | It decreases with the introduction of a catalyst |
| D. | It increases with increase of temperature |
| Answer» E. | |
| 1193. |
The experimental data for the reaction \[2A+{{B}_{2}}\to 2AB\] is [CBSE PMT 1997] Exp. \[{{[A]}_{0}}\] \[{{[B]}_{0}}\] Rate (mole \[{{s}^{-1}}\]) (1) 0.50 0.50 \[1.6\times {{10}^{-4}}\] (2) 0.50 1.00 \[3.2\times {{10}^{-4}}\] (3) 1.00 1.00 \[3.2\times {{10}^{4}}\] The rate equation for the above data is |
| A. | Rate \[=k\,[{{B}_{2}}]\] |
| B. | Rate \[=k\,{{[{{B}_{2}}]}^{2}}\] |
| C. | Rate \[=k{{[A]}^{2}}\,{{[B]}^{2}}\] |
| D. | Rate \[=k\,{{[A]}^{2}}[B]\] |
| Answer» B. Rate \[=k\,{{[{{B}_{2}}]}^{2}}\] | |
| 1194. |
Half life period of a first order reaction is 138.6 minutes. The velocity constant of the reaction is |
| A. | \[0.05\,{{\min }^{-1}}\] |
| B. | \[0.00005\,{{\min }^{-1}}\] |
| C. | \[0.005\,{{\min }^{-1}}\] |
| D. | \[200\,{{\min }^{-1}}\] |
| Answer» D. \[200\,{{\min }^{-1}}\] | |
| 1195. |
The time of half change of a first order reaction in ....... initial concentration |
| A. | Proportional to |
| B. | Inversely proportional to |
| C. | Independent of |
| D. | Equal to |
| Answer» D. Equal to | |
| 1196. |
If ?a? is the initial concentration and ?n? is the order of the reaction and the half life period is ?T?, then [MH CET 2000] |
| A. | \[T\propto {{a}^{n-1}}\] |
| B. | \[T\propto {{a}^{n}}\] |
| C. | \[T\propto \frac{1}{{{a}^{n}}}\] |
| D. | \[T\propto \frac{1}{{{a}^{n-1}}}\] |
| Answer» E. | |
| 1197. |
For a zero order reaction |
| A. | The concentration of the reactant does not change during the reaction |
| B. | The concentration change only when the temperature changes |
| C. | The rate remains constant throughout |
| D. | The rate of the reaction is proportional to the concentration |
| Answer» D. The rate of the reaction is proportional to the concentration | |
| 1198. |
For reation, \[A+B\to \] products, it is found that the rate of the reaction is proportional to the concentration of A, but it is independent of the concentration of B, then |
| A. | The order of the reaction 2 and molecularity 1 |
| B. | Molecularity of the reaction is 2 but order is 1 |
| C. | Order is 2 and molecularity is 2 |
| D. | Order of the reaction is 2 but molecularity is 0 |
| Answer» C. Order is 2 and molecularity is 2 | |
| 1199. |
The velocity constant of first order reaction is expressed in the units |
| A. | Concentration per unit time |
| B. | Time per unit concentration |
| C. | Per unit time |
| D. | Unit time per unit concentration |
| Answer» D. Unit time per unit concentration | |
| 1200. |
If the half life period of a reaction is inversely proportional to the initial concentration, the order of the reaction is |
| A. | Zero |
| B. | One |
| C. | Two |
| D. | Three |
| Answer» D. Three | |