Explanation Given information : For benzene: a = 18.0 L 2 atm / mole 2 and b = 0.1154 L / mole Calculation: Let us consider the ideal gas law for a gas at low temperature and pressure as shown below P V = n R T Here, P is the pressure (in atm), V is the volume (in L), T is the temperature (in K), n is the number of moles of the gas, And the molar gas constant R = 0.0820578. Now, consider the Van der Waals equation which covers the non-ideal case as shown below ( P + n 2 a V 2 ) ( V − n b ) = n R T And consider the following parameters values T = 700 K P = 20 atm a = 18.0 L 2 -atm/mole 2 b = 0.1154 L / mole n = 1 Let us find the volume of 1 mole of benzene with given parameters. Now, find out initial guess from the ideal gas law as shown below. V = n R T P = 1 × 0.0820578 × 320 15 = 2.872023 L Let us consider the following function. f ( V ) = ( P + n 2 a V 2 ) ( V − n b ) − n R T = ( 20 + 18

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ISBN: 9780134696454

Author: Sauer, Tim

Publisher: Pearson,

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Chapter 1.4, Problem 12CP

To determine

The volume of 1 mole of benzene vapour at 700 K under a pressure of 20 atm.

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Chapter 1.4, Problem 11CP

Chapter 1.4, Problem 13CP

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