At ${10}^{°}C$ the value of the density of a fixed mass of an ideal gas divided by its pressure is x. At ${110}^{°}C$ this ratio is 

(a) x

(b)$\frac{383}{283}x$

(c)$\frac{10}{110}x$

(d) $\frac{283}{383}x$

Which of the following is not thermodynamical function ?

(1) Enthalpy

(2) Work done

(3) Gibb's energy

(4) Internal energy

Which of the following is not a thermodynamics co-ordinate ?

(1) P

(2) T

(3) V

(4) R

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

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

In an isothermal change, an ideal gas obeys -

(1) Boyle's law

(2) Charle's law

(3) Gaylussac law

(4) None of the above

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

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 ΔU_I and ΔU_II are the changes in internal energies in the processes I and II respectively, then 

(1) ΔU_II > ΔU_I

(2) ΔU_II < ΔU_I

(3) ΔU_I = ΔU_II

(4) Relation between ΔU_I and ΔU_II can not be determined