70 calories of heat is required to raise the temperature of 2 moles of an ideal gas at constant pressure from 30°C to 35°C. The amount of heat required to raise the temperature of same gas through the same range (30°C to 35°C) at constant volume (R = 2 cal/mol/K)

1.  30 cal                       

2.  50 cal

3.  70 cal                       

4.  90 cal

Subtopic:  Specific Heat |
 74%
From NCERT
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A closed compartment containing gas is moving with some acceleration in horizontal direction. Neglect effect of gravity. Then the pressure in the compartment is

1. Same everywhere                           

2. Lower in the front side

3. Lower in the rear side                     

4. Lower in the upper side

Subtopic:  Kinetic Energy of an Ideal Gas |
From NCERT
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Three closed vessels A, B and C are at the same temperature T and contain gases which obey the Maxwellian distribution of velocities. Vessel A contains only O2 , B only N2 and C a mixture of equal quantities of O2 and N2. If the average speed of the O2 molecules in vessel A is V1 , that of the N2 molecules in vessel B is V2 , the average speed of the O2 molecules in vessel C is

1. V1+V2/2                           

2. V1

3. V1V21/2                               

4. 3 kT/M

Subtopic:  Types of Velocities |
From NCERT
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A box containing N molecules of a perfect gas at temperature T1 and pressure P1. The number of molecules in the box is doubled keeping the total kinetic energy of the gas same as before. If the new pressure is P2 and temperature T2, then

1. P2=P1, T2=T1                           

2. P2=P1, T2=T12

3. P2=2P1, T2=T1                         

4. P2=2P1, T2=T12

Subtopic:  Kinetic Energy of an Ideal Gas |
From NCERT
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Two identical glass bulbs are interconnected by a thin glass tube. A gas is filled in these bulbs at N.T.P. If one bulb is placed in ice and another bulb is placed in hot bath, then the pressure of the gas becomes 1.5 times. The temperature of hot bath will be

      

1.  100°C                     

2.  182°C

3.  256°C                     

4.  546°C

Subtopic:  Ideal Gas Equation |
From NCERT
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Two containers of equal volumes contain the same gas at pressures \(P_1\) and \(P_2\) and absolute temperatures \(T_1\) and \(T_2\), respectively. On joining the vessels, the gas reaches a common pressure \(P\) and common temperature \(T\). The ratio \(\frac{P}{T}\) is equal to:
1. \(\frac{P_1}{T_1}+\frac{P_2}{T_2}\)
2. \(\frac{P_1T_1+P_2T_2}{(T_1+T_2)^2}\)
3. \(\frac{P_1T_2+P_2T_1}{(T_1+T_2)^2}\)
4. \(\frac{P_1}{2T_1}+\frac{P_2}{2T_2}\)

Subtopic:  Ideal Gas Equation |
 52%
From NCERT
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At the top of a mountain a thermometer reads 7°C and a barometer reads 70 cm of Hg. At the bottom of the mountain these read 27°C and 76 cm of Hg respectively. Comparison of density of air at the top with that of bottom is

   
1.  75/76                             

2.  70/76

3.  76/75                             

4.  76/70

Subtopic:  Ideal Gas Equation |
 65%
From NCERT
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A vessel is partitioned in two equal halves by a fixed diathermic separator. Two different ideal gases are filled in left (L) and right (R) halves. The rms speed of the molecules in L part is equal to the mean speed of molecules in the R part. Then the ratio of the mass of a molecule in L part to that of a molecule in R part is

1. 32                           

2. π4

3. 23                           

4. 3π8

Subtopic:  Types of Velocities |
 68%
From NCERT
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A gas is filled in the cylinder shown in the figure. The two pistons are joined by a string. If the gas is heated, the pistons will

1.Move towards left                 

2. Move towards right

3. Remain stationary                 

4. None of these

Subtopic:  Ideal Gas Equation |
 56%
From NCERT
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A closed vessel contains 8gm of oxygen and 7gm of nitrogen. The total pressure is 10 atm at a given temperature. If now oxygen is absorbed by introducing a suitable absorbent the pressure of the remaining gas in atm will be

1.  2                               

2.  10

3.  4                               

4.  5

Subtopic:  Ideal Gas Equation |
 69%
From NCERT
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