B-5. (A) 2.24 litre (B) 0.020 mL (C) 2.24 mL (U12 For the non-zero values of force of attraction between gas molecules, gas equation will be (A) PV = nRT (B) PV = nRT +'nbP (C) PV = nRT V-b a"ח (D) P= nRT

For non-zero value of force of attraction between gas molecular at large volume, gas equation will be : (a) PV=nRT-(n^(2)a)/(V) (b) PV=nRT+nbP (c) P=(nRT)/(V-b) (d) PV=nRT

Which of the following indicates Kinetic gas equation ? a) PV = (3M)/(C^2) " " b) PV = 1/3 mnC^2 " " c) P = 1/3 dC^3 " " d) KE = 3/2 RT

Units of a and b in van der Waal's equation (P+(an^(2))/(V^(2)))(V-nb)=nRT are

Units of a and b in van der Waal's equation (P+(an^(2))/(V^(2)))(V-nb)=nRT are

A real gas obeying van der Waals' equation : ( P + ( an^(2))/( V^(2))) ( V - b ) = nRT will closely resemble an ideal gas if

Why is the correction term (n^2 a)/V^2 in the van der Waal's equation [p+(n^2 a)/V^2] (V-n b)=nRT . positive?

Ideal gas equation is represented as PV=nRT . Gases present in universe were fond ideal in the Boyle's temperature range only and deviated more from ideal gas behavior at high pressure and low temperature. The deviation are explained in term of compressibility factor z . For ideal behavior Z=(PV)/(nRT)=1 . the main cause to show deviavtion were due to wrong assumptions made about forces oif attractions (which becomes significant at high pressure ) and volume V occupied by molecules in PV=nRT is supposed to be volume of gas or the volume of container in which gas is placed by assuming that gaseous molecules do not have appreciable volume. Actually volume of the gas is that volume in which each molecule of gas can move freely. If volume occupied by gaseous molecule is not negligible, then the term V would be replaced by the ideal volume which by available for free motion of each molecule of gas in 1 mole gas. V_("actual")= volume of container -volume occupied by molecules =v-b Where b represent the excluded volume occupied by molecules present in one mole of gas. Similarly for n mole gas V_("actual")=v-nb The ratio of coefficient of thermal expansion alpha=(((delV)/(delT))_(P))/V and the isothermal compressibility beta=-((delV)/(delP)_(T)) for an ideal gas is:

Ideal gas equation is represented as PV=nRT . Gases present in universe were fond ideal in the Boyle's temperature range only and deviated more from ideal gas behavior at high pressure and low temperature. The deviation are explained in term of compressibility factor z . For ideal behavior Z=(PV)/(nRT)=1 . the main cause to show deviavtion were due to wrong assumptions made about forces oif attractions (which becomes significant at high pressure ) and volume V occupied by molecules in PV=nRT is supposed to be volume of gas or the volume of container in which gas is placed by assuming that gaseous molecules do not have appreciable volume. Actually volume of the gas is that volume in which each molecule of gas can move freely. If volume occupied by gaseous molecule is not negligible, then the term V would be replaced by the ideal volume which by available for free motion of each molecule of gas in 1 mole gas. V_("actual")= volume of container -volume occupied by molecules =v-b Where b represent the excluded volume occupied by molecules present in one mole of gas. Similarly for n mole gas V_("actual")=v-nb The ratio of coefficient of thermal expansion alpha=(((delV)/(delT))_(P))/V and the isothermal compressibility beta=-((delV)/(delP)_(T)) for an ideal gas is: