One mole of a monoatomic gas is heated at a constant pressure of 1 atmosphere from 0 K to 100 K. If the gas constant R = 8.32J/mol K, the change in internal energy of the gas is approximately:
2.3 J
46 J
8.67 x 103 J
1.25 x 103 J
5.6 litre of helium gas at STP is adiabatically compressed to 0.7 litre. Taking the initial temperature to be T1, the work done in the process is:
A Carnot engine operating between temperatures T1 and T2 has efficiency 1/6. When T2 is lowered by 62 K, its efficiency increases to 1/3. Then T1 and T2 are, respectivley:
372 K and 310 K
372 K and 330 K
330 K and 268 K
310 K and 248 K
Which one is correct ?
In an isobaric process, ΔP = 0
In an isochoric process, ΔW = 0
In an isothermal process, ΔT = 0
In an isothermal process, ΔQ = 0
In thermodynamic processes which of the following statements is not true?
In an adiabatic process the system is insulated from the surroundings
In an isochoric process pressure remains constant
In an isothermal process the temperature remains constant
In an adiabatic process pVγ = constant
One mole of an ideal gas at an initial temperature of T K does 6R joules of work adiabatically. If the ratio of specific heats of this gas at constant pressure and at constant volume is 5/3, the final temperature of gas will be:
(T + 2.4)K
(T - 2.4)K
(T + 4)K
(T - 4)K
A gas is suddenly compressed to 1/4th of its original volume at normal temperature. The increase in its temperature (γ = 1.5) is:
273 K
573 K
373 K
473 K
Universal gas constant is:
CP - CV
CP + CV
An ideal gas is taken through the cycle A B C A as shown in the figure. If the net heat supplied to the gas in the cycle is 5 J, the work done by the gas in the process C A is:
- 5 J
- 10 J
- 15 J
- 20 J
1 g of water at atmospheric pressure has a volume of 1 cm3 and when boiled it becomes 1681 cm3 of steam. The heat of vaporisation of water is 540 cal/g. Then the change in its internal energy in this process is :
540 cal
500 cal
1681 cal
none of these
