Now, look at the Z versus P curve for ethane (Figure 7.6 in textbook) and think

ID: 475131 • Letter: N

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Now, look at the Z versus P curve for ethane (Figure 7.6 in textbook) and think about your answers to questions 2 and 3 above. In this figure, Z first decreases and then rises. Explain this change in terms of intermolecular forces and the van der Waals parameters a and b. Hit, which van der Waal factor dominates in which region and why? Write COMPLETE sentences. Complete the table. Sketch figure 705. Add krypton to this picture. Does it look more like ethane or hydrogen? Why? This is just derivative practice. Another equation of state is the Berthelot equation: RT = (p + a/Tv^2) (v -b) For this equation, calculate a.

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6. When Z< 1, Z is decreasing with increasing pressure that means attractive intermolecular forces dominate & when Z > 1, Z is increasing with pressure that means repulsive intermolecular forces dominate.

When Z< 1 that means (P+ a/Tv2)(V - b) is lower that means a is decreasing and B is increasing leading to overall product to be lower.

When Z > 1 that means a is increasing and b is decreasing leading to overall product to be higher.

Molecular pair Largest a value Intermolecular force Largest b value F2 or B2 London dispersion force H2O or H2S H2O Hydrogen bond Methane London dispersion force Ne or Xe London dispersion force Xe NH3 Hydrogen bond

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Now, look at the Z versus P curve for ethane (Figure 7.6 in textbook) and think

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