The quantitative relationship between the vapor pressure `p` of a liquid and the absolute temperature `T` is given by the Clausius - Clapeyron equation,
`In_(p) = - (Delta_(vap)H)/(RT) + C`
where `In` is the natural logarithm , `R` is the gas constant `(8.314 JK^(-1) mol^(-))` , and `C` is a constant . The plot of

For the reaction , X(s) harr Y(s) + Z(g) , the plot of ln (pz)/p^(theta) versus 10^4/T is given below (in solid line), where p_z is the pressure (in bar) of the gas at temperature T and p^(theta) = 1bar ( Given, (d(lnK))/(d(1/T))= - (DeltaH^(theta))/R , where the equilibrium constant , K= p_z/p^(theta) and the gas constant, R=8.314 JK^(-1)mol^(-1) The value of DeltaS^(theta) (in jmol^(-1) ) for the given reaction at 1000K is ---------

For the reaction , X(s) harr Y(s) + Z(g) , the plot of ln (pz)/p^(theta) versus 10^4/T is given below (in solid line), where p_z is the pressure (in bar) of the gas at temperature T and p^(theta) = 1bar ( Given, (d(lnK))/(d(1/T))= - (DeltaH^(theta))/R , where the equilibrium constant , K= p_z/p^(theta) and the gas constant, R=8.314 JK^(-1)mol^(-1) The value of standard enthalpy, DeltaH^(theta) (in kjmol^(-1) ) for the given reaction is ---------

"m" is the mass of a molecule, "k" is the Boltzmann constant, P is the pressure and T is the absolute temperature. The density of the gas is given by

m is the mass of a molecule, k is he Boltzmann constant,p is the pressure and T is the absolute temperature.The density of the gas is given by?

Find out the unit and dimensions of the constants a and b in the van der Waal's equation ( P + (a)/(V^(2))) ( V - b ) = R t , where P is pressure , v is volume , R is gas constant , and T is temperature.

The pressure P of a gas is plotted against its absolute temperature T for two different constant volumes, V_(1) and V_(2) (for same no. of moles) where V_(1) gt V_(2) , the correct statement is: