In: Chemistry
For the following process, use a calculation to predict whether or not it will occur spontaneously.
A piston with radius of 10.0 cm containing 4.00 L of an ideal gas (Cv,m = 3/2 R) at 1.03 atm, 298.15 K undergoes isothermal expansion when a 4.63 kg weight that was sitting on the piston was quickly removed.
Given:- The radius of the base of the piston, r = 10.0 cm
Also, 1 cm = 0.01 m
So, r = 0.1 m
The area of the base of the piston, A can be calculated as:-
So,
The force acting due to the weight is:-
So, Force, F can be calculated as:-
The pressure due to this weight can be calculated as:-
The expression for the conversion of pressure in Pascal to pressure in atm is shown below:
Given the value of pressure = 1445.1257 Pa
So,
Pressure = 0.01426 atm
Given, Atmospheric pressure=1.03 atm
So, Initial pressure = 1.03 + 0.01426 atm = 1.04426 atm
The weight is removed.
So, Final pressure = 1.03 atm
Also,
Using ideal gas equation as:
where,
P is the pressure = 1.04426 atm
V is the volume = 4.00 L
n is the number of moles
T is the temperature = 298.15 K
R is Gas constant having value = 0.0821 L.atm/K.mol
Applying the equation as:
1.04426 atm × 4.00 L = n × 0.0821 L.atm/K.mol × 298.15 K
⇒n = 0.1706 moles
The expression for the calculation of entropy change for isothermal expansion of the ideal gas is:-
Where, R is the gas constant (8.314 J /mol K)
So,
Also,
The expression for the standard change in free energy is:
Where,
is the change in the Gibbs free energy.
T is the absolute temperature. (T in kelvins)
is the enthalpy change of the reaction.
is the change in entropy.
For isothermal expansion of an ideal gas,
So,
Also, For a system to be spontaneous,
Thus, must be positive for the system to be spontaneous.
(Positive) and thus, the system is spontaneous.