A solution contains 4.08 g of chloroform (CHCl3) and 9.29 g of acetone (CH3COCH3). The vapor pressures at 35 ∘C of pure chlorofo
rm and pure acetone are 295 torr and 332 torr, respectively. Assuming ideal behavior, calculate the vapor pressures of each of the components and the total vapor pressure above the solution.
2 answers:
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Complete Question
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Answer
a
As the valve is opened , the gas will flow into the empty container until the both containers have the same pressure
b
c
The driving force for this process is the increase in entropy this is because the movement of the internal energy of the gas into a larger volume, what this does is that it increases the amount of disorder(entropy).
Explanation
In order to obtain the parameter in the part B of the question we are first obtain the initial pressure, using the ideal gas equation
The next thing is to obtain the new pressure of the gas , using boyle's law
Since the this process is isothermal , the change in heat is equal to zero
i.e q = 0 J
The workdone to move the gas to the other container is zero because the the pressure at this second container is zero due to the fact that it is a vacuum
i.e
Since the change in heat is zero and the workdone is zero then the change in internal energy is equal to 0
This is because the change in internal energy is equal to a summation of change in heat and the workdone
i.e
Generally the change in enthalpy is mathematically represented as
Since the temperature is zero this means that the change in temperature is zero , substituting this value for change in temperature into the equation for change in enthalpy
