Which one of the following statements is not correct about the three states of matter e. solid, liquid and gaseous

The temperature and pressure at which ice, liquid water and water vapour can exist together are

(A) 0º C, 1 atm                                               (B) 2º C, 4.7 atm
(C) 0º C, 4.7 mm                                            (D) -2º C, 4.7 atm

Which of the following is true about gaseous state

Kinetic energy of molecules is highest in

Which of the following statement is correct

A volume of 1 m³ is equal to

(A) 1000 cm³                         (B) 100 cm³                        (C) 10 dm³                         (D) 10⁶ cm³

Which one of the following is not a unit of pressure

1º C rise in temperature is equal to a rise of

(A) 1º F                     (B) 9/5º F                    (C) 5/9º F                    (D) 33º F

Which of the following relations for expressing volume of a sample is not correct

(A) 1 L = 10³ ml                                       (B) 1 dm³ = 1 L

(C) 1 L = 10³  m³                                     (D) 1 L = 10³ cm³

The temperature at which Celsius and Fahrenheit scales give the same reading is

(A) 0^o  C             (B) 32º F                   (C) -40º C                     (D) 40º C

One atmosphere is numerically equal to approximately

(A) 10⁶ dynes  cm^-2              (B) 10² dynes  cm^-2                 (C) 10⁴ dynes  cm^-2             (D) 10⁸ dynes  cm^-2

Torr is a unit of

Pressure of a gas in a vessel can be measured by

A temperature of shall be equal to

(A) 233 K                         (B) -40º F                       (C) -32º F                         (D) Both (a) and (b)

Volume occupied by a gas at one atmospheric pressure and 0º C is V mL. Its volume at 273 K will be

(A) V ml                                                  (B) V/2 ml
(C) 2V                                                     (D) None of these

Which one of the following statements is wrong for gases

If P, V, T represent pressure, volume and temperature of the gas, the correct representation of Boyle’s law is

(A)  V   (at constant p)                                           (B)  PV = RT
(C)  V ∝ 1/P (at constant 7)                                     (D)  PV = nRT

At constant temperature, in a given mass of an ideal gas

Air at sea level is dense. This is a practical application of

If 20 cm³ gas at 1 atm. is expanded to 50 cm³ at constant T, then what is the final pressure

(A) 
(B)   
(C) 
(D)  None Of These

A gas of volume 100 cc is kept in a vessel at pressure 10⁴ Pa maintained at temperature 24ºC  . If now the pressure is increased to 10⁵ Pa, keeping the temperature constant, then the volume of the gas becomes

Which of the following statement is false

Which of the following graphs represent Boyle’s law

(A)  

(B)  

(C)  

(D)  

Densities of two gases are in the ratio 1 : 2 and their temperatures are in the ratio 2 : 1, then the ratio of their respective pressures is

If pressure becomes double at the same absolute temperature on 2 L, then the volume of CO₂ becomes

At constant pressure, the volume of fixed mass of an ideal gas is directly proportional to

Which of the following expression at constant pressure represents Charle’s law

(A)  V                              (B)  V                            (C)  V ∝ T                            (D)  V ∝ d

Use of hot air balloons in sports and meteorological obsevations is an application of

A 10 g of a gas at atmospheric pressure is cooled from 273º C to 0º C  keeping the volume constant, its pressure would become

At what temperature in the Celsius scale, V (volume) of a certain mass of gas at 27º C will be doubled keeping the pressure constant

(A) 54º C                                      (B) 327º C                                  (C) 427º C                                    (D) 527º C

Volume of the air that will be expelled from a vessel of 300 cm³  when it is heated from 27º C  to 37º C  at the same pressure will be

(A 310 cm³                   (B) 290 cm³                       (C) 10 cm³                       (D) 37 cm³

Pressure remaining the same, the volume of a given mass of an ideal gas increases for every degree centigrade rise in temperature by definite fraction of its volume at

The following graph illustrates

A certain sample of gas has a volume of 0.2 litre measured at 1 atm. pressure and . At the same pressure but at , its volume will be

300 ml of a gas at 27º C  is cooled to -3º C  at constant pressure, the final volume is

400 cm³ of oxygen at 27º C were cooled to -3º C without change in pressure. The contraction in volume will be

(A) 40 cm³                    (B) 30 cm³                      (C) 44.4 cm³                     (D) 360 cm³

The pressure p of a gas is plotted against its absolute temperature T for two different constant volumes, V₁ and V₂ . When V₁ > V₂  , 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 V₂ has a greater slope than that for V₁

(D) Curve for V₁ has a greater slope than that for V₂

Vibrational energy is

Two closed vessels of equal volume containing air at pressure P₁ and temperature T₁ are connected to each other through a narrow tube. If the temperature in one of the vessels is now maintained at T₁  and that in the other at T₂ , what will be the pressure in the vessels

(A)                   (B) 

(C)                  (D) 

“One gram molecule of a gas at N.T.P. occupies 22.4 litres.” This fact was derived from

In a closed flask of 5 litres, 1.0 g of H₂  is heated from 300 to 600 K. which statement is not correct

Which one of the following statements is false

(A) Avogadro number = 6.02 × 10²¹
(B) The relationship between average velocity (ν) and root mean square velocity (u) is ν = 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)½

The compressibility of a gas is less than unity at STP. Therefore

(A) V_m > 22.4 liters                                        (B) V_m < 22.4 liters
(C) V_m = 22.4 liters                                        (D) V_m = 44.8 liters

The number of moles of any gas is given by

(A) n/V                       (B) nN_A                                (C) N/N_A                             (D) mnN_A

In the ideal gas equation, the gas constant R has the dimensions of

In the equation PV = nRT , which one cannot be the numerical value of R

(A) 8.31 × 10⁷ ergK^-1 mol^-1                                    (B)  8.31 × 10⁷ dyne cmK^-1 mol^-1

(C)  8.31 JK^-1 mol^-1                                                      (D)  8.31 atm.K^-1 mol^-1

Which one of the following indicates the value of the gas constant R

The constant R is

Select one correct statement. In the gas equation,

The correct value of the gas constant R is close to

(A) 0.082 litre-atmosphere K 
(B) 0.082 litre-atmosphere K^-1 mol^-1
(C) 0.082 litre-atmosphere ^-1 K  mole^-1     
(D) 0.082 litre^-1atmosphere ^-1 K mol^-1 

S.I. unit of gas constant R is

(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

Gas equation PV = nRT  is obeyed by

For an ideal gas number of moles per litre in terms of its pressure P, gas constant R and temperature T is

If the pressure and absolute temperature of 2 litres of CO₂ are doubled, the volume of CO₂ would become  

If two moles of an ideal gas at 546 K occupy a volume of 44.8 litres, the pressure must be

The volume of 1 g each of methane (CH₄) , ethane (C₂H₆) , propane (C₃H₈) and butane (C₄H₁₀)  was measured at 350 K and 1 atm. What is the volume of butane 

(A) 495 cm³                      (B) 600 cm³                       (C) 900 cm³                      (D) 1700 cm³

How many moles of He gas occupy 22.4 litres at  and one atmospheric pressure

Volume of 0.5 mole of a gas at 1 atm. pressure and  is

Pressure of a mixture of 4 g of O₂ and 2 g of H₂ confined in a bulb of 1 litre at Oº C is

At 0º 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

When helium is allowed to expand into vacuum, heating effect is observed. Its reason is that

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 

16 g of oxygen and 3 g of hydrogen are mixed and kept at 760 mm pressure and 0º C . The total volume occupied by the mixture will be nearly

Pure hydrogen sulphide is stored in a tank of 100 liter capacity at 20º C and 2 atm pressure. The mass of the gas will be   

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 273ºC

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 liter of the same gas weigh one gram

A wheather balloon filled with hydrogen at 1 atm and 27ºC has volume equal to 12000 litres. On ascending it reaches a place where the temperature is -23ºC and pressure is 0.5 atm. The volume of the balloon is

The density of a gas at 27ºC and 1 atm is d. Pressure remaining constant at which of the following temperatures will its density become 0.75 d 

(A) 20ºC                                        (B) 30ºC                                  (C) 400                                          (D) 300 K

A sample of gas occupies 100 ml at 27ºC and 740 mm pressure. When its volume is changed to 80 ml at 740 mm pressure, the temperature of the gas will be 

(A) 21.6º C                       (B) 240º C                         (C) -33º C                         (D) 89.5ºC

In an experiment during the analysis of a carbon compound, 145 cm³ of H₂  was collected at 760 mm Hg pressure and 27ºC temperature. The mass of H₂ is nearly  

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

“Equal volumes of all gases at the same temperature and pressure contain equal number of particles.” This statement is a direct consequence of   

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 

(A) P = P_A + P_B + P_C
(B)
(C)
(D) None

Dalton’s law of partial pressure will not apply to which of the following mixture of gases

(A) H₂ and SO₂                             (B) H₂ and Cl₂                      (C) H₂ and CO₂                        (D) CO₂ and Cl₂

Which of the following mixtures of gases does not obey Dalton’s law of partial pressure

(A) O₂ and CO₂                                 (B) N₂ and O₂                                            (C) Cl₂ and O₂                                   (D) NH₃ and HCl

A sample of O₂  gas is collected over water at 23º C at a barometric pressure of 751 mm Hg (vapour pressure of water at23º C is 21 mm Hg). The partial pressure of O₂  gas in the sample collected is

Equal volumes of two gases which do not react together are enclosed in separate vessels. Their pressures at 100 mm and 400 mm respectively. If the two vessels are joined together, then what will be the pressure of the resulting mixture (temperature remaining constant)

To which of the following gaseous mixtures is Dalton’s law not applicable

(A) Ne + He + SO₂                                                       (B) NH₃ + HCl + HBr
(C) O₂ + N₂ + CO₂                                                        (D) N₂ + H₂ + O₂

Same mass of CH₄ and H₂ is taken in container. The partial pressure caused by H₂ is

(A)                              (B)
(C)                             (D) 1

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

Rate of  diffusion of a gas is

Which of the following gas will have highest rate of diffusion

(A) NH₃                           (B) N₂                          (C) CO₂                             (D) O₂

Which of the following relationship is correct, where r is the rate of diffusion of a gas and d is its density

(A) r
(B) r
(C) r = d
(D) r ∝ d

According to Grahman’s law at a given temperature, the ratio of the rates of diffusion r_A/r_B  of gases A and B is given by

(A) (P_A/P_B)(M_A/M_B)½                                    (B) (M_A/M_B)(P_A/P_B)½
(C) (P_A/P_B)(M_B/M_A)½                                    (D) (M_A/M_B)(P_B/P_A)½

(where P and M are the pressures and molecular weights of gases A and B respectively)

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

The rate of diffusion of SO₂ and O₂ are in the ratio

(A)                       (B)1 : 32           (C) 1 : 2                   (D)1 : 4

A gas diffuse 1/5 times as fast as hydrogen. Its molecular weight is

(A) 50
(B) 25
(C)
(D)

The molecular weight of a gas which diffuses through a porous plug at 1/6th of the speed of hydrogen under identical conditions is

Molecular weight of a gas that diffuses twice as rapidly as the gas with molecular weight 64 is

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

If rate of diffusion of A is 5 times that of B, what will be the density ratio of A and B

50 ml of hydrogen diffuses out through a small hole from a vessel in 20 minutes. The time needed for 40 ml of oxygen to diffuse out is

The densities of two gases are in the ratio of 1 : 16. The ratio of their rates of diffusion is

At constant volume and temperature conditions, the rate of diffusion D_A and D_B of gases A and B having densities P_A and P_B are related by the expression

(A)
(B)
(C)
(D)

Atmolysis is a process of

A bottle of ammonia and a bottle of dry hydrogen chloride connected through a long tube are opened simultaneously at both ends, the white ammonium chloride ring first formed will be

Which of the following pairs will diffuse at the same rate through a porous plug

(A) CO, NO₂                                                 (B) NO₂, CO₂
(C) NH₃, PH₃                                               (D) NOC₂H₆

If 4 g of oxygen diffuse through a very narrow hole, how much hydrogen would have diffused under identical conditions

A gas diffuse at a rate which is twice that of another gas B. The ratio of molecular weights of A to B is

Two grams of hydrogen diffuse from a container in 10 minutes. How many grams of oxygen would diffuse through the same container in the same time under similar conditions

A closed vessel contains equal number of nitrogen and oxygen molecules at a pressure of P mm. If nitrogen is removed from the system then the pressure will be

The ratio of rates of diffusion of SO₂, O₂ and CH₄ is

(A) 1 : √2 : 2                                       (B) 1: 2 : 4
(C) 2 : √2 : 1                                       (D) 1 : 2 : √2

The rate of diffusion of methane at a given temperature is twice that of X. The molecular weight of X is

X ml H₂  of  gas effuses through a hole in a container in 5 seconds. The time taken for the effusion of the same volume of the gas specified below under identical condition is

(A) 10 seconds : He                            (B) 20 seconds : O₂
(C) 25 seconds : CO                           (D) 55 seconds : CO₂

At what temperature, the rate of effusion of N₂ would be 1.625 times that of SO₂ at 50º C

Given the reaction C(s) + H₂O(l) → CO(g) + H₂(g) calculate the volume of the gases produced at STP from 48.0 g of carbon

Postulate of kinetic theory is

According to kinetic theory of gases,

In deriving the kinetic gas equation, use is made of the root mean square velocity of the molecules because it is

Kinetic energy of a gas depends upon its

The kinetic theory of gases perdicts that total kinetic energy of a gaseous assembly depends on

According to kinetic theory of gases, the energy per mole of a gas is equal to

Internal energy and pressure of a gas per unit volume are related as

At what temperature will the average speed of CH₄ molecules have the same value as O₂  has at 300 K

The translational kinetic energy of an ideal gas depends only on its

Helium atom is two times heavier than a hydrogen molecule at 298 K, the average kinetic energy of helium is

Which of the following is valid at absolute zero

If a gas is expanded at constant temperature

The average K.E. of an ideal gas in calories per mole is approximately equal to

According to kinetic theory of gases, for a diatomic molecule

At STP, 0.50 mol H₂ gas and 1.0 mol He gas

At the same temperature and pressure, which of the following gases will have the highest kinetic energy per mole

Indicate the correct statement for a 1-L sample of N₂(g) and CO₂(g) at 298 K and 1 atm pressure

(A) The average translational KE per molecule is the same in N₂ and CO₂
(B) The rms speed remains constant for both N₂ and CO₂
(C) The density of  N₂  is less than that of  CO₂
(D) The total translational KE of both N₂ and CO₂ is the same 

With increase of pressure, the mean free path

Consider the following statements

 The mean free path of gas molecules

(1) Decreases with increase in concentration

(2) Increases with decrease in pressure at constant temperature

(3) Decreases with increase in molecular size

The ratio of root mean square velocity to average velocity of gas molecules at a particular temperature is

Which is not true in case of an ideal gas

If C₁, C₂, C₃…… represent the speeds of n₁, n₂, n_3…… molecules, then the root mean square speed is

(A)

(B)

(C)

(D)

The ratio among most probable velocity, mean velocity and root mean square velocity is given by

(A) 1 : 2 : 3                                        

(B) 1 : √2 : √3

(C)                                         

(D)

What is the relationship between the average velocity (v), root mean square velocity (u) and most probable velocity (a)

(A) ∝ : ν : µ : 1 : 1.128 : 1.224                           (B) ∝ : ν : µ :: 1.128 : 1 : 1.224
(C) ∝ : ν : µ :: 1.128 : 1.224 : 1                          (D) ∝ : ν : µ ::1.124 : 1.228 : 1

Which of the following has maximum root mean square velocity at the same temperature

(A) SO₂                                    (B) CO₂                                      (C) O₂                                           (D) H₂

The temperature at which RMS velocity of SO₂ molecules is half that of He molecules at 300 K is

At 27º C , the ratio of rms velocities of ozone to oxygen is

(A)
(B)
(C)
(D) 0.25

The average kinetic energy of an ideal gas per molecule in SI units at 25º C will be

(A) 6.17 × 10^-21 kJ                                 (B) 6.17 × 10^-21 J
(C) 6.17 × 10^-20 J                                   (D) 7.16 × 10^-20 J

At what temperature the RMS velocity of SO₂ be same as that of O₂ at 303 K

Among the following gases which one has the lowest root mean square velocity at 25º C

(A) SO₂                                        (B) N₂                                      (C) O₂                                         (D) Cl₂

The root mean square velocity of an ideal gas in a closed container of fixed volume is increased from 5 × 10⁴ cm s^-1 to 10 × 10⁴ cm s^-1. Which of the following statement correctly explains how the change is accomplished

The rms velocity at NTP of the species can be calculated from the expression

(A)
(B)
(C)
(D) All The Above

Root mean square velocity of a gas molecule is proportional to

(A) m½                     (B) m⁰                           (C) m^-½                        (D) m

At constant volume, for a fixed number of moles of a gas, the pressure of the gas increases with increase in temperature due to

The root mean square speeds at STP for the gases H₂ , N₂ , O₂ and HBr are in the order

(A) H₂ < N₂ < O₂ < HBr                                      (B) HBr < O₂ < N₂ < H₂
(C) H₂ < N₂ < O₂ = HBr                                      (D) HBr < O₂ < H₂ < N₂

A bottle of cold drink contains 200 ml liquid in which CO₂ is 0.1 molar. Suppose CO₂ behaves like an ideal gas, the volume of the dissolved CO₂ at STP is

The temperature of the gas is raised from 27º C to 927º C , the root mean square velocity is

(A) times the earlier value        
(B) Same as before
(C) Halved
(D) Doubled

The ratio between the root mean square velocity of H₂ at 50 K and that of O₂ at 800 K is

The root mean square velocity of an ideal gas at constant pressure varies density (d) as

(A) d²                                (B) d                           (C)  √d                          (D) 1/√d

Consider a mixture of SO₂ and O₂ kept at room temperature. Compared to the oxygen molecule, the SO₂  molecule will hit the wall with

The rms speed of N₂ molecules in a gas is u. If the temperature is doubled and the nitrogen molecules dissociate into nitrogen atoms, the rms speed becomes

Consider the following statements : For diatomic gases, the ratio  is equal to

(1) 1.40 (lower temperature)

(2) 1.66 (moderate temperature)

(3) 1.29 (higher temperature)

Which of the above statements are correct

The Vander Waal’s equation explains the behaviour of

Gases deviate from the ideal gas behaviour because their molecules

The compressibility factor of a gas is defined as Z = PV/RT. The compressibility factor of ideal gas is

In Vander Waal’s equation of state for a non-ideal gas, the term that accounts for intermolecular forces is

(A) (V-b)                                     (B) (RT)^-1                       

(C)                         (D) RT

Vander Waal’s equation of state is obeyed by real gases. For n moles of a real gas, the expression will be

(A)

(B)

(C)

(D)

Any gas shows maximum deviation from ideal gas at 

(A) 0^oC and 1 atmospheric pressure                        (B)  100^oC and 2 atmospheric pressure         

(C) -100^oC and 5 atmospheric pressure                  (D)  500^oC and 1 atmospheric pressure

The temperature at which the second virial coefficient of real gas is zero is called

When is deviation more in the behaviour of a gas from the ideal gas equation PV = nRT