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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.
| 1201. |
Decay constant of a reaction is \[1.1\times {{10}^{-9}}/\sec \], then the half life of the reaction is |
| A. | \[1.2\times {{10}^{8}}\] |
| B. | \[6.3\times {{10}^{8}}\] |
| C. | \[3.3\times {{10}^{8}}\] |
| D. | \[2.1\times {{10}^{8}}\] |
| Answer» C. \[3.3\times {{10}^{8}}\] | |
| 1202. |
The data for the reaction \[A+B\to C\] is [CBSE PMT 1994] Exp. \[{{[A]}_{0}}\] \[{{[B]}_{0}}\] Initial rate (1) 0.012 0.035 0.10 (2) 0.024 0.070 0.80 (3) 0.024 0.035 0.10 (4) 0.012 0.070 0.80 The rate law corresponds to the above data is |
| A. | Rate \[=k\,{{[B]}^{3}}\] |
| B. | Rate \[=k\,{{[B]}^{4}}\] |
| C. | Rate \[=k\,[A]\,{{[B]}^{3}}\] |
| D. | Rate \[=\,k\,{{[A]}^{2}}\,{{[B]}^{2}}\] |
| Answer» B. Rate \[=k\,{{[B]}^{4}}\] | |
| 1203. |
The order of a reaction is said to be 2 with respect to a reactant X, when [DPMT 2000] |
| A. | The rate of the reaction is proportional to [X] |
| B. | The rate of the reaction is proportional \[{{[X]}^{2}}\] |
| C. | Two molecules of X are present in the stoichiometric equation |
| D. | The reaction occurs in two steps |
| Answer» C. Two molecules of X are present in the stoichiometric equation | |
| 1204. |
The half life period of a first order reaction [AMU 2000] |
| A. | \[\frac{0.693}{t}\] |
| B. | \[\frac{0.693}{K}\] |
| C. | \[\frac{2.303}{t}\] |
| D. | \[\frac{0.303}{{{K}_{1}}}\] |
| Answer» C. \[\frac{2.303}{t}\] | |
| 1205. |
A first order reaction requires 30 minutes for 50% completion. The time required to complete the reaction by 75% will be |
| A. | 45 minutes |
| B. | 15 minutes |
| C. | 60 minutes |
| D. | None of these |
| Answer» D. None of these | |
| 1206. |
Inversion of canesugar in dilute acid (conversion into glucose and fructose) is a |
| A. | Unimolecular reaction |
| B. | Bimolecular reaction |
| C. | Trimolecular reaction |
| D. | Pseudo-unimolecular reaction |
| Answer» E. | |
| 1207. |
The unit of specific reaction rate constant for a first order (if the concentration expressed in molarity) would be [MNR 1988; UPSEAT 2000, 01] |
| A. | mole \[litr{{e}^{-1}}{{s}^{-1}}\] |
| B. | mole \[litr{{e}^{-1}}\] |
| C. | mole \[{{s}^{-1}}\] |
| D. | \[{{s}^{-1}}\] |
| Answer» E. | |
| 1208. |
The half life of a first order reaction is |
| A. | Independent of the initial concentration of the reactant |
| B. | Directly proportional to the initial concentration of the reactants |
| C. | Inversely proportional to the initial concentration of the reactant |
| D. | Directly proportional to the square of the initial concentration of the reactant |
| Answer» B. Directly proportional to the initial concentration of the reactants | |
| 1209. |
By ?the overall order of a reaction?, we mean |
| A. | The number of concentration terms in the equation for the reaction |
| B. | The sum of powers to which the concentration terms are raised in the velocity equation |
| C. | The least number of molecules of the reactants needed for the reaction |
| D. | The number of reactants which take part in the reaction |
| Answer» C. The least number of molecules of the reactants needed for the reaction | |
| 1210. |
Catalyst decomposition of hydrogen peroxide is a ........ order reaction |
| A. | First |
| B. | Second |
| C. | Third |
| D. | Zero |
| Answer» B. Second | |
| 1211. |
\[A+2B\to C+D\]. If \[-\frac{d[A]}{dt}=5\times {{10}^{-4}}mol\,{{l}^{-1}}{{s}^{-1}}\]1, then \[-\frac{d[B]}{dt}\] is [DPMT 2005] |
| A. | \[2.5\times {{10}^{-4}}mol\,{{l}^{-1}}{{s}^{-1}}\] |
| B. | \[5.0\times {{10}^{-4}}mol\,{{l}^{-1}}{{s}^{-1}}\] |
| C. | \[2.5\times 10-3mol\,{{l}^{-1}}{{s}^{-1}}\] |
| D. | \[1.0\times {{10}^{-3}}mol\,{{l}^{-1}}{{s}^{-1}}\] |
| Answer» B. \[5.0\times {{10}^{-4}}mol\,{{l}^{-1}}{{s}^{-1}}\] | |
| 1212. |
A reaction involving two different reactants [KCET 1989; AIEEE 2005] |
| A. | Can never be a second order reaction |
| B. | Can never be a unimolecular reaction |
| C. | Can never be a bimolecular reaction |
| D. | Can never be a first order reaction |
| Answer» C. Can never be a bimolecular reaction | |
| 1213. |
The reaction \[2{{N}_{2}}{{O}_{5}}\]⇌\[2N{{O}_{2}}+{{O}_{2}}\] follows first order kinetics. Hence, the molecularity of the reaction is |
| A. | Unimolecular |
| B. | Pseudo?unimolecular |
| C. | Bimolecular |
| D. | None of the above |
| Answer» D. None of the above | |
| 1214. |
The order of a reaction which has the rate expression \[\frac{dc}{dt}=K{{[E]}^{3/2}}{{[D]}^{3/2}}\] is |
| A. | 3/2 |
| B. | 3 |
| C. | 2 |
| D. | 0 |
| Answer» C. 2 | |
| 1215. |
A first order reaction which is 30% complete in 30 minutes has a half-life period of [AIIMS 1998] |
| A. | 24.2 min |
| B. | 58.2 min |
| C. | 102.2 min |
| D. | 120.2 min |
| Answer» C. 102.2 min | |
| 1216. |
The first order rate constant for the decomposition of \[{{N}_{2}}{{O}_{5}}\] is \[6.2\times {{10}^{-4}}{{\sec }^{-1}}\]. The half life period for this decomposition in seconds is [MNR 1991; MP PET 1997; UPSEAT 2000] |
| A. | 1117.7 |
| B. | 111.7 |
| C. | 223.4 |
| D. | 160.9 |
| Answer» B. 111.7 | |
| 1217. |
Which one of the following formula represents a first order reaction [MP PMT 1999] |
| A. | \[K=\frac{x}{t}\] |
| B. | \[K=\frac{1}{2t}\left[ \frac{1}{{{(a-x)}^{2}}}-\frac{1}{{{a}^{2}}} \right]\] |
| C. | \[K=\frac{2.303}{t}{{\log }_{10}}\frac{a}{(a-x)}\] |
| D. | \[K=\frac{1}{t}\,\frac{x}{a(a-x)}\] |
| Answer» D. \[K=\frac{1}{t}\,\frac{x}{a(a-x)}\] | |
| 1218. |
The inversion of cane sugar is represented by \[{{C}_{12}}{{H}_{22}}{{O}_{11}}+{{H}_{2}}O\to {{C}_{6}}{{H}_{12}}{{O}_{6}}+{{C}_{6}}{{H}_{12}}{{O}_{6}}\] It is a reaction of [AFMC 1982; MP PMT 1993; RPET 2000] |
| A. | Second order |
| B. | Unimolecular |
| C. | Pseudo unimolecular |
| D. | None of the three |
| Answer» D. None of the three | |
| 1219. |
Which of the following is a first order reaction [MP PMT 1987] |
| A. | \[N{{H}_{4}}N{{O}_{2}}\to {{N}_{2}}+2{{H}_{2}}O\] |
| B. | \[2HI\]\[\to \]\[{{H}_{2}}+{{I}_{2}}\] |
| C. | \[2N{{O}_{2}}\to 2NO+{{O}_{2}}\] |
| D. | \[2NO+{{O}_{2}}\to 2N{{O}_{2}}\] |
| Answer» B. \[2HI\]\[\to \]\[{{H}_{2}}+{{I}_{2}}\] | |
| 1220. |
The rate of reaction between \[A\] and \[B\] increases by a factor of 100, when the concentration of \[A\] is increased 10 folds. The order of reaction with respect to \[A\] is [CPMT 1985] |
| A. | 10 |
| B. | 1 |
| C. | 4 |
| D. | 2 |
| Answer» E. | |
| 1221. |
The hydrolysis of ethyl acetate is a reaction of [MP PMT 1987] \[C{{H}_{3}}COOEt+{{H}_{2}}O\xrightarrow{{{H}^{+}}}C{{H}_{3}}COOH+EtOH\] |
| A. | First order |
| B. | Second order |
| C. | Third order |
| D. | Zero order |
| Answer» B. Second order | |
| 1222. |
The following data are for the decomposition of ammonium nitrate in aqueous solution Volume of \[{{N}_{2}}\] in cc Time (minutes) 6.25 10 9.50 15 11.42 20 13.65 25 35.05 Finally The order of the reaction is [NCERT 1980] |
| A. | Zero |
| B. | One |
| C. | Two |
| D. | Three |
| Answer» C. Two | |
| 1223. |
For a chemical reaction \[A\to B\] it is found that the rate of reaction doubles, when the concentration of A is increased four times. The order in A for this reaction is [NCERT 1979; AIIMS 1997; J & K CET 2005] |
| A. | Two |
| B. | One |
| C. | Half |
| D. | Zero |
| Answer» D. Zero | |
| 1224. |
The rate law for the reaction Sucrose + Water \[\xrightarrow{[{{H}^{+}}]}\] Glucose + Fructose is given by |
| A. | Rate \[=K\] [sucrose] [water] |
| B. | Rate \[=K\] [sucrose] [water]\[^{0}\] |
| C. | Rate \[=K\] [sucrose]\[^{0}\][water] |
| D. | Rate \[=K\] [sucrose]\[^{1/2}\] [water]\[^{1/2}\] |
| Answer» C. Rate \[=K\] [sucrose]\[^{0}\][water] | |
| 1225. |
The rates of a certain reaction (dc/dt) at different times are as follows Time Rate (mole litre?1 sec ?1 ) 0 \[2.8\times {{10}^{-2}}\] 10 \[2.78\times {{10}^{-2}}\] 20 \[2.81\times {{10}^{-2}}\] 30 \[2.79\times {{10}^{-2}}\] The reaction is [NCERT 1978] |
| A. | Zero order |
| B. | First order |
| C. | Second order |
| D. | Third order |
| Answer» B. First order | |
| 1226. |
The unit of rate constant for a zero order reaction is [NCERT 1981; MP PMT 2000; RPET 2000] |
| A. | litre \[{{\sec }^{-1}}\] |
| B. | litre \[mol{{e}^{-1}}\,{{\sec }^{-1}}\] |
| C. | mole \[litr{{e}^{-1}}{{\sec }^{-1}}\] |
| D. | mole \[{{\sec }^{-1}}\] |
| Answer» D. mole \[{{\sec }^{-1}}\] | |
| 1227. |
A zero order reaction is one whose rate is independent of [NCERT 1981] |
| A. | Temperature of the reaction |
| B. | The concentrations of the reactants |
| C. | The concentration of the products |
| D. | The material of the vessel in which the reaction is carried out |
| Answer» C. The concentration of the products | |
| 1228. |
The unit of rate constant of second order reaction is usually expressed as [NCERT 1983, 84; MNR 1983; MP PMT 1994, 99] |
| A. | mole litre \[{{\sec }^{-1}}\] |
| B. | \[mol{{e}^{-1}}\,litr{{e}^{-1}}{{\sec }^{-1}}\] |
| C. | \[mole\,litr{{e}^{-1}}\,{{\sec }^{-1}}\] |
| D. | \[mol{{e}^{-1}}\,litre\,{{\sec }^{-1}}\] |
| Answer» E. | |
| 1229. |
The dimension of rate constant of a second order reaction involves [NCERT 1982] |
| A. | Neither time nor concentration |
| B. | Only time |
| C. | Time and concentration |
| D. | Time and square of concentration |
| Answer» D. Time and square of concentration | |
| 1230. |
If the concentration is expressed in moles per litre, the unit of the rate constant for a first order reaction is [MNR 1986; MP PET 1994, 2000, 01;Bihar MEE 1996; CPMT 1997; MP PMT 1995, 96, 99;AFMC 2002] |
| A. | mole litre \[^{-1}\,{{\sec }^{-1}}\] |
| B. | mole litre\[^{-1}\] |
| C. | \[{{\sec }^{-1}}\] |
| D. | mole\[^{-1}\] litre\[^{-1}\] sec\[^{-1}\] |
| Answer» D. mole\[^{-1}\] litre\[^{-1}\] sec\[^{-1}\] | |
| 1231. |
The specific rate constant of a first order reaction depends on the [IIT 1981, 83; DPMT 1991; Bihar MEE 1995; KCET 1998] |
| A. | Concentration of the reactants |
| B. | Concentration of the products |
| C. | Time of reaction |
| D. | Temperature of reaction |
| Answer» E. | |
| 1232. |
The rate equation for the reaction \[2A+B\to C\] is found to be: rate \[=k[A][B]\]. The correct statement in relation to this reaction is that the [AIEEE 2004] |
| A. | Rate of formation of C is twice the rate of disappearance of A |
| B. | \[{{t}_{1/2}}\]is a constant |
| C. | Unit of k must be \[{{s}^{-1}}\] |
| D. | Value of k is independent of the initial concentrations of A and B |
| Answer» E. | |
| 1233. |
In the reaction \[2{{N}_{2}}{{O}_{5}}\to 4N{{O}_{2}}+{{O}_{2}}\], initial pressure is \[500\,atm\] and rate constant \[K\] is \[3.38\times {{10}^{-5}}{{\sec }^{-1}}\]. After 10 minutes the final pressure of \[{{N}_{2}}{{O}_{5}}\] is [Orissa JEE 2005] |
| A. | 490 atm |
| B. | 250 atm |
| C. | 480 atm |
| D. | 420 atm |
| Answer» B. 250 atm | |
| 1234. |
The value of rate constant \[A+B\to \] products depends on [BHU 2003] |
| A. | Concentration of A and B |
| B. | Pressure |
| C. | Temperature |
| D. | All of these |
| Answer» D. All of these | |
| 1235. |
The rate constant of a reaction depends upon [BHU 2004] |
| A. | Extent of reaction |
| B. | Time of reaction |
| C. | Temperature of the system |
| D. | Concentration of the system |
| Answer» D. Concentration of the system | |
| 1236. |
If \[R=K{{[NO]}^{2}}[{{O}_{2}}],\] rate constant may be increased by [BHU 2003] |
| A. | Increasing temperature |
| B. | Decreasing temperature |
| C. | Increasing concentration of \[{{O}_{2}}\] |
| D. | Increasing concentration of \[NO\] |
| Answer» B. Decreasing temperature | |
| 1237. |
The rate law of the reaction \[2{{N}_{2}}{{O}_{5}}\to 4N{{O}_{2}}+{{O}_{2}}\] is [MP PET 2002] |
| A. | \[r=K[{{N}_{2}}{{O}_{5}}]\] |
| B. | \[r=K{{[{{N}_{2}}{{O}_{5}}]}^{2}}\] |
| C. | \[r=K{{[{{N}_{2}}{{O}_{5}}]}^{0}}\] |
| D. | \[r=K{{[N{{O}_{2}}]}^{4}}[{{O}_{2}}]\] |
| Answer» B. \[r=K{{[{{N}_{2}}{{O}_{5}}]}^{2}}\] | |
| 1238. |
For the reaction \[2{{N}_{2}}{{O}_{5}}\to 4N{{O}_{2}}+{{O}_{2}}\]rate of reaction and rate constant are \[1.02\times {{10}^{-4}}\]and \[3.4\times {{10}^{-5}}{{\sec }^{-1}}\] respectively. The concentration of \[{{N}_{2}}{{O}_{5}}\] at that time will be [BHU 2001] |
| A. | \[1.732\] |
| B. | 3 |
| C. | \[1.02\times {{10}^{-4}}\] |
| D. | \[3.4\times {{10}^{5}}\] |
| Answer» C. \[1.02\times {{10}^{-4}}\] | |
| 1239. |
A reaction that is of the first order with respect to reactant A has a rate constant \[6{{\min }^{-1}}.\] If we start with \[[A]=0.5\,mol\,\,{{l}^{-1}}\], when would \[[A]\]reach the value 0.05mol \[{{l}^{-1}}\] [KCET 2000] |
| A. | 0.384 min |
| B. | 0.15 min |
| C. | 3 min |
| D. | 3.84 min |
| Answer» B. 0.15 min | |
| 1240. |
The rate constant for the reaction, \[2{{N}_{2}}{{O}_{5}}\to 4N{{O}_{2}}\]\[+{{O}_{2}}\] is \[3\times {{10}^{-5}}{{\sec }^{-1}}\]. If the rate is \[2.40\times {{10}^{-5}}mol\,\,litr{{e}^{\text{-1}}}{{\sec }^{-1}}\]. Then the concentration of \[{{N}_{2}}{{O}_{5}}\](in mol litre-1) is [IIT Screening 2000] |
| A. | 1.4 |
| B. | 1.2 |
| C. | 0.04 |
| D. | 0.8 |
| Answer» E. | |
| 1241. |
The reaction \[{{N}_{2}}{{O}_{5}}\,(\text{in}\,CC{{l}_{4}}\,\text{solution})\to 2N{{O}_{2}}(\text{solution})+\frac{1}{2}{{O}_{2}}(g)\] is of first order in \[{{N}_{2}}{{O}_{5}}\] with rate constant \[6.2\times {{10}^{-1}}{{s}^{-1}}.\] What is the value of rate of reaction when \[[{{N}_{2}}{{O}_{5}}]=1.25\,mole\,{{l}^{-1}}\] [AFMC 1998] |
| A. | \[7.75\times {{10}^{-1}}mole\,{{l}^{-1}}{{s}^{-1}}\] |
| B. | \[6.35\times {{10}^{-3}}mole\,{{l}^{-1}}{{s}^{-1}}\] |
| C. | \[5.15\times {{10}^{-5}}mole\,{{l}^{-1}}{{s}^{-1}}\] |
| D. | \[3.85\times {{10}^{-1}}mole\,{{l}^{-1}}\,{{s}^{-1}}\] |
| Answer» B. \[6.35\times {{10}^{-3}}mole\,{{l}^{-1}}{{s}^{-1}}\] | |
| 1242. |
Rate constant for a reaction \[{{H}_{2}}+{{I}_{2}}\to 2HI\] is 49, then rate constant for reaction \[2HI\to {{H}_{2}}+{{I}_{2}}\] is [Bihar MEE 1997] |
| A. | 7 |
| B. | 1/49 |
| C. | 49 |
| D. | 21 |
| E. | 63 |
| Answer» C. 49 | |
| 1243. |
The rate of the reaction \[CC{{l}_{3}}CHO+NO\to CHC{{l}_{3}}+NO+CO\] is given by Rate \[=K\,[CC{{l}_{3}}CHO]\,[NO]\]. If concentration is expressed in moles/litre, the units of K are [MP PET 1993] |
| A. | \[litr{{e}^{2}}\,mol{{e}^{-2}}\,{{\sec }^{-1}}\] |
| B. | \[mole\,litr{{e}^{-1}}{{\sec }^{-1}}\] |
| C. | \[litre\,mol{{e}^{-1}}{{\sec }^{-1}}\] |
| D. | \[{{\sec }^{-1}}\] |
| Answer» D. \[{{\sec }^{-1}}\] | |
| 1244. |
The rate law for reaction \[A+2B=C+2D\] will be |
| A. | Rate \[=K[A]\,[B]\] |
| B. | Rate \[=K[A]\,[2B]\] |
| C. | Rate \[=K[A]\,{{[B]}^{2}}\] |
| D. | Rate \[=K\frac{[C]{{[D]}^{2}}}{[A]{{[B]}^{2}}}\] |
| Answer» D. Rate \[=K\frac{[C]{{[D]}^{2}}}{[A]{{[B]}^{2}}}\] | |
| 1245. |
The rate of reaction is determined by slow step reaction. The step is called |
| A. | Reaction rate |
| B. | Activation step |
| C. | Rate determining step |
| D. | None of the above |
| Answer» D. None of the above | |
| 1246. |
Which of the following oxides of nitrogen will be the most stable one [NCERT 1978] |
| A. | \[2N{{O}_{2}}(g)\]⇌\[{{N}_{2}}(g)+2{{O}_{2}}(g);K=6.7\times {{10}^{16}}mol\,{{l}^{-1}}\] |
| B. | \[2NO(g)\]⇌ \[{{N}_{2}}(g)+{{O}_{2}}(g);\,K=2.2\times {{10}^{30}}mol\,{{l}^{-1}}\] |
| C. | \[2{{N}_{2}}{{O}_{5}}(g)\]⇌\[2{{N}_{2}}(g)+5{{O}_{2}}(g);\,K=1.2\times {{10}^{34}}\,mol\,{{l}^{-5}}\] |
| D. | \[2{{N}_{2}}O(g)\]⇌\[2{{N}_{2}}(g)+{{O}_{2}}(g);\,K=3.5\times {{10}^{33}}\,mol\,litr{{e}^{-1}}\] |
| Answer» B. \[2NO(g)\]⇌ \[{{N}_{2}}(g)+{{O}_{2}}(g);\,K=2.2\times {{10}^{30}}mol\,{{l}^{-1}}\] | |
| 1247. |
Which of the following reactions end in finite time [DPMT 2005] |
| A. | 0 order |
| B. | 1st order |
| C. | 2nd order |
| D. | 3rd order |
| Answer» B. 1st order | |
| 1248. |
For the reaction \[A+B\to C\], it is found that doubling the concentration of A increases the rate by 4 times, and doubling the concentration of B doubles the reaction rate. What is the overal order of the reaction. [KCET 2005] |
| A. | 4 |
| B. | 3/2 |
| C. | 3 |
| D. | 1 |
| Answer» D. 1 | |
| 1249. |
The half-life of a first order reaction having rate constant K = 1.7 ´ 10-5 s-1 is [BHU 2005] |
| A. | 12.1 h |
| B. | 9.7 h |
| C. | 11.3 h |
| D. | 1.8 h |
| Answer» D. 1.8 h | |
| 1250. |
If a substance with half life 3 days is taken at other place in 12 days. What amount of substance is left now [AFMC 2005] |
| A. | 1/4 |
| B. | 1/8 |
| C. | 1/16 |
| D. | 1/32 |
| Answer» D. 1/32 | |