At the value of the density of a fixed mass of an ideal gas divided by its pressure is x. At this ratio is
Writing ideal gas law
Which of the following is not thermodynamical function ?
(2) Work done
(3) Gibb's energy
(4) Internal energy
(2) Work done is not a thermodynamical function.
Which of the following is not a thermodynamics co-ordinate ?
(4) R is the universal gas constant.
Which of the following statements is correct for any thermodynamic system ?
(1) The internal energy changes in all processes
(2) Internal energy and entropy are state functions
(3) The change in entropy can never be zero
(4) The work done in an adiabatic process is always zero
(2) The internal energy and entropy depend only on the initial and final states of the system and not on the path followed to attain that state.
A monoatomic gas of n-moles is heated from temperature T1 to T2 under two different conditions (i) at constant volume and (ii) at constant pressure. The change in internal energy of the gas is
(1) More for (i)
(2) More for (ii)
(3) Same in both cases
(4) Independent of number of moles
(3) Change in internal energy
it doesn’t depend upon type of process. Actually it is a state function
In an isothermal change, an ideal gas obeys -
(1) Boyle's law
(2) Charle's law
(3) Gaylussac law
(4) None of the above
(1) In isothermal process, compressibility Eθ = ρ.
A gas mixture consists of 2 moles of oxygen and 4 moles argon at temperature T. Neglecting all vibrational modes, the total internal energy of the system is
(1) 4 RT
(2) 15 RT
(3) 9 RT
(4) 11 RT
(4) Oxygen is diatomic gas, hence its energy of two moles
Argon is a monoatomic gas, hence its internal energy of 4 moles
Total Internal energy = (6 + 5)RT = 11RT
Which one of the following gases possesses the largest internal energy ?
(1) 2 moles of helium occupying 1m3 at 300 K
(2) 56 kg of nitrogen at Nm–2 and 300 K
(3) 8 grams of oxygen at 8 atm and 300 K
(4) 6 × 1026 molecules of argon occupying 40 m3 at 900 K
A system goes from A to B via two processes I and II as shown in figure. If ΔUI and ΔUII are the changes in internal energies in the processes I and II respectively, then
(1) ΔUII > ΔUI
(2) ΔUII < ΔUI
(3) ΔUI = ΔUII
(4) Relation between ΔUI and ΔUII can not be determined
(3) As internal energy is a state function therefore change in internal energy does not depends upon the path followed i.e.