van der Waal's equation for calculating the pressure of a non ideal gas is
`(P+(an^(2))/(V^(2)))(V-nb)=nRT`
van der Waal's suggested that the pressure exerted by an ideal gas , `P_("ideal")`, is related to the experiventally measured pressure, `P_("ideal")` by the equation
`P_("ideal")=underset("observed pressure")(underset(uarr)(P_("real")))+underset("currection term")(underset(uarr)((an^(2))/(V^(2))))`
Constant 'a' is measure of intermolecular interaction between gaseous molecules that gives rise to nonideal behavior. It depends upon how frequently any two molecules approach each other closely. Another correction concerns the volume occupied by the gas molecules. In the ideal gas equation, V represents the volume of the container. However, each molecule does occupy a finite, although small, intrinsic volume, so the effective volume of the gas vecomes (V-nb), where n is the number of moles of the gas and b is a constant. The term nb represents the volume occupied by gas particles present in n moles of the gas .
Having taken into account the corrections for pressure and volume, we can rewrite the ideal gas equation as follows :
`underset("corrected pressure")((P+(an^(2))/(V^(2))))underset("corrected volume")((V-nb))=nRT`
The van der Waals' constant 'a' for `CO_(2)` gas is greater than that of `H_(2)` gas. Its mean that the
van der Waal's equation for calculating the pressure of a non ideal gas is
`(P+(an^(2))/(V^(2)))(V-nb)=nRT`
van der Waal's suggested that the pressure exerted by an ideal gas , `P_("ideal")`, is related to the experiventally measured pressure, `P_("ideal")` by the equation
`P_("ideal")=underset("observed pressure")(underset(uarr)(P_("real")))+underset("currection term")(underset(uarr)((an^(2))/(V^(2))))`
Constant 'a' is measure of intermolecular interaction between gaseous molecules that gives rise to nonideal behavior. It depends upon how frequently any two molecules approach each other closely. Another correction concerns the volume occupied by the gas molecules. In the ideal gas equation, V represents the volume of the container. However, each molecule does occupy a finite, although small, intrinsic volume, so the effective volume of the gas vecomes (V-nb), where n is the number of moles of the gas and b is a constant. The term nb represents the volume occupied by gas particles present in n moles of the gas .
Having taken into account the corrections for pressure and volume, we can rewrite the ideal gas equation as follows :
`underset("corrected pressure")((P+(an^(2))/(V^(2))))underset("corrected volume")((V-nb))=nRT`
The van der Waals' constant 'a' for `CO_(2)` gas is greater than that of `H_(2)` gas. Its mean that the
`(P+(an^(2))/(V^(2)))(V-nb)=nRT`
van der Waal's suggested that the pressure exerted by an ideal gas , `P_("ideal")`, is related to the experiventally measured pressure, `P_("ideal")` by the equation
`P_("ideal")=underset("observed pressure")(underset(uarr)(P_("real")))+underset("currection term")(underset(uarr)((an^(2))/(V^(2))))`
Constant 'a' is measure of intermolecular interaction between gaseous molecules that gives rise to nonideal behavior. It depends upon how frequently any two molecules approach each other closely. Another correction concerns the volume occupied by the gas molecules. In the ideal gas equation, V represents the volume of the container. However, each molecule does occupy a finite, although small, intrinsic volume, so the effective volume of the gas vecomes (V-nb), where n is the number of moles of the gas and b is a constant. The term nb represents the volume occupied by gas particles present in n moles of the gas .
Having taken into account the corrections for pressure and volume, we can rewrite the ideal gas equation as follows :
`underset("corrected pressure")((P+(an^(2))/(V^(2))))underset("corrected volume")((V-nb))=nRT`
The van der Waals' constant 'a' for `CO_(2)` gas is greater than that of `H_(2)` gas. Its mean that the
A
strength of van der Waals' force of `CO_(2)` gas is less than that of `H_(2)` gas
B
strength of van der Waals' force of `CO_(2)` gas is equal to that of `H_(2)` gas
C
`CO_(2)` gas can be more easily liquified
D
`H_(2)` gas can be more easily liquified
Text Solution
Verified by Experts
The correct Answer is:
c
(c) van der Waal's constant 'a'`prop`I.M.A.F. So `CO_(2)` gas can be more easily liquified.
Topper's Solved these Questions
Similar Questions
Explore conceptually related problems
van der Waal's equation for calculating the pressure of a non ideal gas is (P+(an^(2))/(V^(2)))(V-nb)=nRT van der Waal's suggested that the pressure exerted by an ideal gas , P_("ideal") , is related to the experiventally measured pressure, P_("ideal") by the equation P_("ideal")=underset("observed pressure")(underset(uarr)(P_("real")))+underset("currection term")(underset(uarr)((an^(2))/(V^(2)))) Constant 'a' is measure of intermolecular interaction between gaseous molecules that gives rise to nonideal behavior. It depends upon how frequently any two molecules approach each other closely. Another correction concerns the volume occupied by the gas molecules. In the ideal gas equation, V represents the volume of the container. However, each molecule does occupy a finite, although small, intrinsic volume, so the effective volume of the gas vecomes (V-nb), where n is the number of moles of the gas and b is a constant. The term nb represents the volume occupied by gas particles present in n moles of the gas . Having taken into account the corrections for pressure and volume, we can rewrite the ideal gas equation as follows : underset("corrected pressure")((P+(an^(2))/(V^(2))))underset("corrected volume")((V-nb))=nRT AT relatively high pressures, the van der Waals' equation of state reduces to
van der Waal's equation for calculating the pressure of a non ideal gas is (P+(an^(2))/(V^(2)))(V-nb)=nRT van der Waal's suggested that the pressure exerted by an ideal gas , P_("ideal") , is related to the experiventally measured pressure, P_("ideal") by the equation P_("ideal")=underset("observed pressure")(underset(uarr)(P_("real")))+underset("currection term")(underset(uarr)((an^(2))/(V^(2)))) Constant 'a' is measure of intermolecular interaction between gaseous molecules that gives rise to nonideal behavior. It depends upon how frequently any two molecules approach each other closely. Another correction concerns the volume occupied by the gas molecules. In the ideal gas equation, V represents the volume of the container. However, each molecule does occupy a finite, although small, intrinsic volume, so the effective volume of the gas vecomes (V-nb), where n is the number of moles of the gas and b is a constant. The term nb represents the volume occupied by gas particles present in n moles of the gas . Having taken into account the corrections for pressure and volume, we can rewrite the ideal gas equation as follows : underset("corrected pressure")((P+(an^(2))/(V^(2))))underset("corrected volume")((V-nb))=nRT For non-zero value of force of attraction between gas moleculer at large volume, gas equation will be :
van der Waal's equation for calculating the pressure of a non ideal gas is (P+(an^(2))/(V^(2)))(V-nb)=nRT van der Waal's suggested that the pressure exerted by an ideal gas , P_("ideal") , is related to the experiventally measured pressure, P_("ideal") by the equation P_("ideal")=underset("observed pressure")(underset(uarr)(P_("real")))+underset("currection term")(underset(uarr)((an^(2))/(V^(2)))) Constant 'a' is measure of intermolecular interaction between gaseous molecules that gives rise to nonideal behavior. It depends upon how frequently any two molecules approach each other closely. Another correction concerns the volume occupied by the gas molecules. In the ideal gas equation, V represents the volume of the container. However, each molecule does occupy a finite, although small, intrinsic volume, so the effective volume of the gas vecomes (V-nb), where n is the number of moles of the gas and b is a constant. The term nb represents the volume occupied by gas particles present in n moles of the gas . Having taken into account the corrections for pressure and volume, we can rewrite the ideal gas equation as follows : underset("corrected pressure")((P+(an^(2))/(V^(2))))underset("corrected volume")((V-nb))=nRT Using van der Waals' equation, find the constant 'a' (in atm L^(2)mol^(-2) ) when two moles of a gas confined in 4 L flask exerts a pressure of 11.0 atmospheres at a temperature of 300 K. The value of b is 0.05 L mol^(-1) .(R = 0.082 atm.L/K mol)
The van der Waal equation of gas is (P + (n^(2)a)/(V^(2))) (V - nb) = nRT
Units of a and b in van der Waal's equation (P+(an^(2))/(V^(2)))(V-nb)=nRT are
van der Waal's equation reduces itself to the ideal gas equation at
The pressure P and volume V of an ideal gas both decreases in a process.
The energy density u/V of an ideal gas is related to its pressure P as
The pressure ( P ) and volume ( V ) of an ideal gas both increase in a process:
At low pressure, the van der Waal's equation become :