Urgent help needed! This is the only information given by the professor. Assumin

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Urgent help needed!

This is the only information given by the professor.

Assuming the van der Waals equation of state applies, consider the following systems at 470 K: 1000 mol of pure methanol in a 300 L vessel 1000 mol of pure propanol in a 300 L vessel Recall that the van der Waals equation has the following form: P = RT/v -b - a/v^2, where a = 9RT_c v_c/8 and b = v_c/3 For each system: How many stable phases are predicted AT EQUILIBRIUM by the equation of state? Estimate the density of each stable phase. Estimate the fraction of the system's mass that will be in each phase. Estimate the equilibrium pressure.

Explanation / Answer

For answering the given questions, we require Tc & vc i.e. critical temp. & critical volume respectively. No table provided to calculate Tc & vc

a. Below the critical temperature (Tc) , the stable states on a given isotherm are divided into two groups. The first group is characterized by relatively small molar volumes--these are liquid states. The second group is characterized by relatively large molar volumes--these are gas states. The liquid and gas states are separated by a set of unstable states. Above the critical temperature, the distinct liquid and gas states cease to exist--there is only a single stable fluid state.

b. Density (mass/vol) of each stable phase can only be calculated by knowing vc

c. Total mass = no. of moles * molecular mass. Again, vc will be required from the Table which is not provided.

d. Equilibrium pressure can be calculated by solving a & b and the putting them in given pressure equation.

Again, for calculating a & b, Tc & vc are required. v in the given pressure equation is 300/1000 L/mol = 0.3/1000 m3/mol.

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