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At ${10}^{\xb0}C$ the value of the density of a fixed mass of an ideal gas divided by its pressure is x. At ${110}^{\xb0}C$ this ratio is

(a) x

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

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

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

NEET - 2008

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Which of the following is not thermodynamical function ?

(1) Enthalpy

(2) Work done

(3) Gibb's energy

(4) Internal energy

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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

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A monoatomic gas of *n*-moles is heated from temperature *T*_{1} to *T*_{2} 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

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In an isothermal change, an ideal gas obeys -

(1) Boyle's law

(2) Charle's law

(3) Gaylussac law

(4) None of the above

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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 *

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Which one of the following gases possesses the largest internal energy** ?**

(1) 2 moles of helium occupying 1*m*^{3 }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 × 10^{26} molecules of argon occupying 40 *m*^{3} at 900 *K*

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A system goes from *A* to *B* via two processes I and II as shown in figure. If Δ*U*_{I} and Δ*U*_{II} are the changes in internal energies in the processes I and II respectively, then

(1) Δ*U*_{II} > Δ*U*_{I}

(2) Δ*U*_{II} < Δ*U*_{I}

(3) Δ*U*_{I} = Δ*U*_{II}

(4) Relation between Δ*U*_{I} and Δ*U*_{II} can not be determined

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