MCQOPTIONS
Saved Bookmarks
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.
| 4651. |
If rate of diffusion of A is 5 times that of B, what will be the density ratio of A and B [AFMC 1994] |
| A. | 1/25 |
| B. | 1/5 |
| C. | 25 |
| D. | 4 |
| Answer» B. 1/5 | |
| 4652. |
The densities of hydrogen and oxygen are 0.09 and 1.44 g \[{{L}^{-1}}\]. If the rate of diffusion of hydrogen is 1 then that of oxygen in the same units will be [RPMT 1994] |
| A. | 4 |
| B. | ¼ |
| C. | 16 |
| D. | 1/16 |
| Answer» C. 16 | |
| 4653. |
Molecular weight of a gas that diffuses twice as rapidly as the gas with molecular weight 64 is [EAMCET 1994] |
| A. | 16 |
| B. | 8 |
| C. | 64 |
| D. | 6.4 |
| Answer» B. 8 | |
| 4654. |
The molecular weight of a gas which diffuses through a porous plug at 1/6th of the speed of hydrogen under identical conditions is [EAMCET 1990] |
| A. | 27 |
| B. | 72 |
| C. | 36 |
| D. | 48 |
| Answer» C. 36 | |
| 4655. |
A gas diffuse 1/5 times as fast as hydrogen. Its molecular weight is [CPMT 1992; Bihar CEE 1982] |
| A. | 50 |
| B. | 25 |
| C. | \[25\sqrt{2}\] |
| D. | \[50\sqrt{2}\] |
| Answer» B. 25 | |
| 4656. |
The ratio of the rate of diffusion of a given element to that of helium is 1.4. The molecular weight of the element is [Kerala PMT 1990] |
| A. | 2 |
| B. | 4 |
| C. | 8 |
| D. | 16 |
| Answer» B. 4 | |
| 4657. |
Which of the following relationship is correct, where r is the rate of diffusion of a gas and d is its density [CPMT 1994] |
| A. | \[r\propto \sqrt{1/d}\] |
| B. | \[r\propto \sqrt{d}\] |
| C. | \[r=d\] |
| D. | \[r\propto d\] |
| Answer» B. \[r\propto \sqrt{d}\] | |
| 4658. |
Which of the following gas will have highest rate of diffusion [Pb. CET Sample paper 1993; CPMT 1990] |
| A. | \[N{{H}_{3}}\] |
| B. | \[{{N}_{2}}\] |
| C. | \[C{{O}_{2}}\] |
| D. | \[{{O}_{2}}\] |
| Answer» B. \[{{N}_{2}}\] | |
| 4659. |
Rate of diffusion of a gas is [IIT 1985; CPMT 1987] |
| A. | Directly proportional to its density |
| B. | Directly proportional to its molecular mass |
| C. | Directly proportional to the square root of its molecular mass |
| D. | Inversely proportional to the square root of its molecular mass |
| Answer» E. | |
| 4660. |
Equal amounts of two gases of molecular weight 4 and 40 are mixed. The pressure of the mixture is 1.1 atm. The partial pressure of the light gas in this mixture is [CBSE PMT 1991] |
| A. | 0.55 atm |
| B. | 0.11 atm |
| C. | 1 atm |
| D. | 0.12 atm |
| Answer» D. 0.12 atm | |
| 4661. |
Which of the following statement is false [BHU 1994] |
| A. | The product of pressure and volume of fixed amount of a gas is independent of temperature |
| B. | Molecules of different gases have the same K.E. at a given temperature |
| C. | The gas equation is not valid at high pressure and low temperature |
| D. | The gas constant per molecule is known as Boltzmann constant |
| Answer» B. Molecules of different gases have the same K.E. at a given temperature | |
| 4662. |
To which of the following gaseous mixtures is Dalton's law not applicable |
| A. | \[Ne+He+S{{O}_{2}}\] |
| B. | \[N{{H}_{3}}+HCl+HBr\] |
| C. | \[{{O}_{2}}+{{N}_{2}}+C{{O}_{2}}\] |
| D. | \[{{N}_{2}}+{{H}_{2}}+{{O}_{2}}\] |
| Answer» C. \[{{O}_{2}}+{{N}_{2}}+C{{O}_{2}}\] | |
| 4663. |
Dalton's law of partial pressure will not apply to which of the following mixture of gases [Bihar MADT 1981] |
| A. | \[{{H}_{2}}\] and \[S{{O}_{2}}\] |
| B. | \[{{H}_{2}}\] and \[C{{l}_{2}}\] |
| C. | \[{{H}_{2}}\] and \[C{{O}_{2}}\] |
| D. | \[{{H}_{2}}\] and \[S{{O}_{2}}\] |
| Answer» C. \[{{H}_{2}}\] and \[C{{O}_{2}}\] | |
| 4664. |
Which of the following mixtures of gases does not obey Dalton's law of partial pressure [CBSE PMT 1996: Kerala PMT 2000] |
| A. | \[{{O}_{2}}\] and \[C{{O}_{2}}\] |
| B. | \[{{N}_{2}}\] and \[{{O}_{2}}\] |
| C. | \[C{{l}_{2}}\] and \[{{O}_{2}}\] |
| D. | \[N{{H}_{3}}\] and HCl |
| Answer» E. | |
| 4665. |
If three unreactive gases having partial pressures \[{{P}_{A}},\,{{P}_{B}}\] and \[{{P}_{C}}\] and their moles are 1, 2 and 3 respectively then their total pressure will be [CPMT 1994] |
| A. | \[P={{P}_{A}}+{{P}_{B}}+{{P}_{C}}\] |
| B. | \[P=\frac{{{P}_{A}}+{{P}_{B}}+{{P}_{C}}}{6}\] |
| C. | \[P=\frac{\sqrt{{{P}_{A}}+{{P}_{B}}+{{P}_{C}}}}{3}\] |
| D. | None |
| Answer» B. \[P=\frac{{{P}_{A}}+{{P}_{B}}+{{P}_{C}}}{6}\] | |
| 4666. |
?Equal volumes of all gases at the same temperature and pressure contain equal number of particles.? This statement is a direct consequence of [Kerala MEE 2002] |
| A. | Avogadro?s law |
| B. | Charle's law |
| C. | Ideal gas equation |
| D. | Law of partial pressure |
| Answer» B. Charle's law | |
| 4667. |
The total pressure exerted by a number of non-reacting gases is equal to the sum of the partial pressures of the gases under the same conditions is known as [CPMT 1986] |
| A. | Boyle's law |
| B. | Charle's law |
| C. | Avogadro's law |
| D. | Dalton's law |
| Answer» E. | |
| 4668. |
A sample of gas occupies 100 ml at \[{{27}^{o}}C\] and 740 mm pressure. When its volume is changed to 80 ml at 740 mm pressure, the temperature of the gas will be [Vellore CMC 1991] |
| A. | \[{{21.6}^{o}}C\] |
| B. | \[{{240}^{o}}C\] |
| C. | \[-{{33}^{o}}C\] |
| D. | \[{{89.5}^{o}}C\] |
| Answer» D. \[{{89.5}^{o}}C\] | |
| 4669. |
The density of a gas at \[{{27}^{o}}C\] and 1 atm is d. Pressure remaining constant at which of the following temperatures will its density become 0.75 d [CBSE PMT 1992] |
| A. | \[{{20}^{o}}C\] |
| B. | \[{{30}^{o}}C\] |
| C. | 400 K |
| D. | 300 K |
| Answer» D. 300 K | |
| 4670. |
One litre of a gas weighs 2 g at 300 K and 1 atm pressure. If the pressure is made 0.75 atm, at which of the following temperatures will one litre of the same gas weigh one gram [CBSE PMT 1992] |
| A. | 450 K |
| B. | 600 K |
| C. | 800 K |
| D. | 900 K |
| Answer» B. 600 K | |
| 4671. |
If 20\[c{{m}^{3}}\] gas at 1 atm. is expanded to 50 \[c{{m}^{3}}\] at constant T, then what is the final pressure [CPMT 1988] |
| A. | \[20\times \frac{1}{50}\] |
| B. | \[50\times \frac{1}{20}\] |
| C. | \[1\times \frac{1}{20}\times 50\] |
| D. | None of these |
| Answer» B. \[50\times \frac{1}{20}\] | |
| 4672. |
At N.T.P. the volume of a gas is found to be 273 ml. What will be the volume of this gas at 600 mm Hg and \[{{273}^{o}}C\] [CPMT 1992] |
| A. | 391.8 mL |
| B. | 380 ml |
| C. | 691.6 ml |
| D. | 750 ml |
| Answer» D. 750 ml | |
| 4673. |
Pure hydrogen sulphide is stored in a tank of 100 litre capacity at \[{{20}^{o}}C\] and 2 atm pressure. The mass of the gas will be [CPMT 1989] |
| A. | 34 g |
| B. | 340 g |
| C. | 282.4 g |
| D. | 28.24 g |
| Answer» D. 28.24 g | |
| 4674. |
16 g of oxygen and 3 g of hydrogen are mixed and kept at 760 mm pressure and \[{{0}^{o}}C\]. The total volume occupied by the mixture will be nearly [Vellore CMC 1991] |
| A. | 22.4 litres |
| B. | 33.6 litres |
| C. | 448 litres |
| D. | 44800 ml |
| Answer» E. | |
| 4675. |
Two separate bulbs contain ideal gases A and B. The density of gas A is twice that of gas B. The molecular mass of A is half that of gas B. The two gases are at the same temperature. The ratio of the pressure of A to that of gas B is [BHU 1994] |
| A. | 2 |
| B. | 1/2 |
| C. | 4 |
| D. | ¼ |
| Answer» D. ¼ | |
| 4676. |
Correct gas equation is [CBSE PMT 1989; CPMT 1991] |
| A. | \[\frac{{{V}_{1}}{{T}_{2}}}{{{P}_{1}}}=\frac{{{V}_{2}}{{T}_{1}}}{{{P}_{2}}}\] |
| B. | \[\frac{{{P}_{1}}{{V}_{1}}}{{{P}_{2}}{{V}_{2}}}=\frac{{{T}_{1}}}{{{T}_{2}}}\] |
| C. | \[\frac{{{P}_{1}}{{T}_{2}}}{{{V}_{1}}}=\frac{{{P}_{2}}{{V}_{2}}}{{{T}_{2}}}\] |
| D. | \[\frac{{{V}_{1}}{{V}_{2}}}{{{T}_{1}}{{T}_{2}}}={{P}_{1}}{{P}_{2}}\] |
| Answer» C. \[\frac{{{P}_{1}}{{T}_{2}}}{{{V}_{1}}}=\frac{{{P}_{2}}{{V}_{2}}}{{{T}_{2}}}\] | |
| 4677. |
At \[{{0}^{o}}C\] and one atm pressure, a gas occupies 100 cc. If the pressure is increased to one and a half-time and temperature is increased by one-third of absolute temperature, then final volume of the gas will be [DCE 2000] |
| A. | 80 cc |
| B. | 88.9 cc |
| C. | 66.7 cc |
| D. | 100 cc |
| Answer» C. 66.7 cc | |
| 4678. |
Volume of 0.5 mole of a gas at 1 atm. pressure and \[273K\] is [EAMCET 1992] |
| A. | 22.4 litres |
| B. | 11.2 litres |
| C. | 44.8 litres |
| D. | 5.6 litres |
| Answer» C. 44.8 litres | |
| 4679. |
How many moles of He gas occupy 22.4 litres at \[{{30}^{o}}C\] and one atmospheric pressure [KCET 1992] |
| A. | 0.90 |
| B. | 1.11 |
| C. | 0.11 |
| D. | 1.0 |
| Answer» B. 1.11 | |
| 4680. |
If two moles of an ideal gas at 546 K occupy a volume of 44.8 litres, the pressure must be [NCERT 1981; JIPMER 1991] |
| A. | 2 atm |
| B. | 3 atm |
| C. | 4 atm |
| D. | 1 atm |
| Answer» B. 3 atm | |
| 4681. |
For an ideal gas number of moles per litre in terms of its pressure P, gas constant R and temperature T is [AIEEE 2002] |
| A. | PT/R |
| B. | PRT |
| C. | P/RT |
| D. | RT/P |
| Answer» D. RT/P | |
| 4682. |
Air at sea level is dense. This is a practical application of [Kerala CEE 2000] |
| A. | Boyle's law |
| B. | Charle's law |
| C. | Avogadro's law |
| D. | Dalton's law |
| Answer» B. Charle's law | |
| 4683. |
Gas equation \[PV=nRT\] is obeyed by [BHU 2000] |
| A. | Only isothermal process |
| B. | Only adiabatic process |
| C. | Both A and B |
| D. | None of these |
| Answer» D. None of these | |
| 4684. |
S.I. unit of gas constant R is [CPMT 1994] |
| A. | 0.0821 litre atm K?1 mole?1 |
| B. | 2 calories K?1 mole?1 |
| C. | 8.31 joule K?1 mole?1 |
| D. | None |
| Answer» D. None | |
| 4685. |
Select one correct statement. In the gas equation, \[PV=nRT\] [CBSE PMT 1992] |
| A. | n is the number of molecules of a gas |
| B. | V denotes volume of one mole of the gas |
| C. | n moles of the gas have a volume V |
| D. | P is the pressure of the gas when only one mole of gas is present |
| Answer» D. P is the pressure of the gas when only one mole of gas is present | |
| 4686. |
The correct value of the gas constant R is close to [CBSE PMT 1992] |
| A. | 0.082 litre-atmopshere K |
| B. | 0.082 litre-atmosphere \[{{K}^{-1}}\,mo{{l}^{-1}}\] |
| C. | 0.082 litre-\[atmospher{{e}^{-1}}\,K\,mol{{e}^{-1}}\] |
| D. | 0.082 \[litr{{e}^{-1}}\,atmospher{{e}^{-1}}\,K\,mol\] |
| Answer» C. 0.082 litre-\[atmospher{{e}^{-1}}\,K\,mol{{e}^{-1}}\] | |
| 4687. |
The constant R is [Orissa 1990] |
| A. | Work done per molecule |
| B. | Work done per degree absolute |
| C. | Work done per degree per mole |
| D. | Work done per mole |
| Answer» D. Work done per mole | |
| 4688. |
Which one of the following indicates the value of the gas constant R [EAMCET 1989] |
| A. | 1.987 cal K?1 mol?1 |
| B. | 8.3 cal K?1 mol?1 |
| C. | 0.0821 lit K?1 mol?1 |
| D. | 1.987 Joules K?1 mol?1 |
| Answer» B. 8.3 cal K?1 mol?1 | |
| 4689. |
In the equation \[PV=nRT\], which one cannot be the numerical value of R [BIT 1987] |
| A. | \[8.31\times {{10}^{7}}erg\,{{K}^{-1}}mo{{l}^{-1}}\] |
| B. | \[8.31\times {{10}^{7}}dyne\,cm\,{{K}^{-1}}mo{{l}^{-1}}\] |
| C. | \[8.31\,J{{K}^{-1}}mo{{l}^{-1}}\] |
| D. | \[8.31\,atm.\,{{K}^{-1}}mo{{l}^{-1}}\] |
| Answer» E. | |
| 4690. |
In the ideal gas equation, the gas constant R has the dimensions of [NCERT 1982] |
| A. | mole-atm K?1 |
| B. | litre mole |
| C. | litre-atm K?1 mole?1 |
| D. | erg K?1 |
| Answer» D. erg K?1 | |
| 4691. |
In the equation of sate of an ideal gas \[PV=nRT\], the value of the universal gas constant would depend only on [KCET 2005] |
| A. | The nature of the gas |
| B. | The pressure of the gas |
| C. | The units of the measurement |
| D. | None of these |
| Answer» D. None of these | |
| 4692. |
The compressibility of a gas is less than unity at STP. Therefore [IIT 2000] |
| A. | \[{{V}_{m}}>22.4\]litres |
| B. | \[{{V}_{m}}<22.4\]litres |
| C. | \[{{V}_{m}}=22.4\]litres |
| D. | \[{{V}_{m}}=44.8\]litres |
| Answer» C. \[{{V}_{m}}=22.4\]litres | |
| 4693. |
At constant temperature, in a given mass of an ideal gas [CBSE PMT 1991] |
| A. | The ratio of pressure and volume always remains constant |
| B. | Volume always remains constant |
| C. | Pressure always remains constant |
| D. | The product of pressure and volume always remains constant |
| Answer» E. | |
| 4694. |
Which one of the following statements is false [Manipal PMT 1991] |
| A. | Avogadro number\[=6.02\times {{10}^{21}}\] |
| B. | The relationship between average velocity \[(\bar{v})\] and root mean square velocity (u) is \[\bar{v}=0.9213\,u\] |
| C. | The mean kinetic energy of an ideal gas is independent of the pressure of the gas |
| D. | The root mean square velocity of the gas can be calculated by the formula \[{{(3RT/M)}^{1/2}}\] |
| Answer» B. The relationship between average velocity \[(\bar{v})\] and root mean square velocity (u) is \[\bar{v}=0.9213\,u\] | |
| 4695. |
In a closed flask of 5 litres, 1.0 g of \[{{H}_{2}}\] is heated from 300 to 600 K. which statement is not correct [CBSE PMT 1991] |
| A. | Pressure of the gas increases |
| B. | The rate of collision increases |
| C. | The number of moles of gas increases |
| D. | The energy of gaseous molecules increases |
| Answer» D. The energy of gaseous molecules increases | |
| 4696. |
?One gram molecule of a gas at N.T.P. occupies 22.4 litres.? This fact was derived from [CPMT 1981, 1995] |
| A. | Dalton's theory |
| B. | Avogadro's hypothesis |
| C. | Berzelius hypothesis |
| D. | Law of gaseous volume |
| Answer» C. Berzelius hypothesis | |
| 4697. |
Two closed vessels of equal volume containing air at pressure \[{{P}_{1}}\] and temperature \[{{T}_{1}}\] are connected to each other through a narrow tube. If the temperature in one of the vessels is now maintained at \[{{T}_{1}}\] and that in the other at \[{{T}_{2}}\], what will be the pressure in the vessels |
| A. | \[\frac{2{{P}_{1}}{{T}_{1}}}{{{T}_{1}}+{{T}_{2}}}\] |
| B. | \[\frac{{{T}_{1}}}{2{{P}_{1}}{{T}_{2}}}\] |
| C. | \[\frac{2{{P}_{1}}{{T}_{2}}}{{{T}_{1}}+{{T}_{2}}}\] |
| D. | \[\frac{2{{p}_{1}}}{{{T}_{1}}+{{T}_{2}}}\] |
| Answer» D. \[\frac{2{{p}_{1}}}{{{T}_{1}}+{{T}_{2}}}\] | |
| 4698. |
The pressure p of a gas is plotted against its absolute temperature T for two different constant volumes, \[{{V}_{1}}\] and \[{{V}_{2}}\]. When \[{{V}_{1}}>{{V}_{2}}\], the |
| A. | Curves have the same slope and do not intersect |
| B. | Curves must intersect at some point other than \[T=0\] |
| C. | Curve for \[{{V}_{2}}\] has a greater slope than that for\[{{V}_{1}}\] |
| D. | Curve for\[{{V}_{1}}\]has a greater slope than that for\[{{V}_{2}}\] |
| Answer» D. Curve for\[{{V}_{1}}\]has a greater slope than that for\[{{V}_{2}}\] | |
| 4699. |
400 \[c{{m}^{3}}\] of oxygen at\[{{27}^{o}}C\]were cooled to \[-{{3}^{o}}C\] without change in pressure. The contraction in volume will be |
| A. | 40 \[c{{m}^{3}}\] |
| B. | 30 \[c{{m}^{3}}\] |
| C. | 44.4 \[c{{m}^{3}}\] |
| D. | 360 \[c{{m}^{3}}\] |
| Answer» B. 30 \[c{{m}^{3}}\] | |
| 4700. |
A certain sample of gas has a volume of 0.2 litre measured at 1 atm. pressure and \[{{0}^{o}}C\]. At the same pressure but at \[{{273}^{o}}C\], its volume will be [EAMCET 1992, 93; BHU 2005] |
| A. | 0.4 litres |
| B. | 0.8 litres |
| C. | 27.8 litres |
| D. | 55.6 litres |
| Answer» B. 0.8 litres | |