Question

3.2 By equating the thermal energy ($k_B T$, where $k_B$ is the Boltzmann constant) with the bonding energy, estimate the temperature at which argon atoms are likely to start to form pairs, and so form a liquid, using the data in question 3.1. Compare this with the boiling point of argon (question 3.22). 3.3 If the atoms in liquid argon are surrounded by 12 nearest neighbours on average, estimate the energy of evaporation of the liquid. 3.4 The Lennard-Jones constants for neon are $A = 4.39 \times 10^{-136} J m^{12}$ and $B = 9.30 \times 10^{-79} J m^6$. Calculate (a) the bonding energy; (b) the equilibrium separation of a pair of neon atoms.

          3.2 By equating the thermal energy ($k_B T$, where $k_B$ is the Boltzmann constant) with the bonding energy, estimate the temperature at which argon atoms are likely to start to form pairs, and so form a liquid, using the data in question 3.1. Compare this with the boiling point of argon (question 3.22).
3.3 If the atoms in liquid argon are surrounded by 12 nearest neighbours on average, estimate the energy of evaporation of the liquid.
3.4 The Lennard-Jones constants for neon are $A = 4.39 \times 10^{-136} J m^{12}$ and $B = 9.30 \times 10^{-79} J m^6$. Calculate (a) the bonding energy; (b) the equilibrium separation of a pair of neon atoms.

3.2 By equating the thermal energy (kB T, where kB is the Boltzmann constant) with the bonding energy, estimate the temperature at which argon atoms are likely to start to form pairs, and so form a liquid, using the data in question 3.1. Compare this with the boiling point of argon (question 3.22).
3.3 If the atoms in liquid argon are surrounded by 12 nearest neighbours on average, estimate the energy of evaporation of the liquid.
3.4 The Lennard-Jones constants for neon are A = 4.39 × 10^-136 J m^12 and B = 9.30 × 10^-79 J m^6. Calculate (a) the bonding energy; (b) the equilibrium separation of a pair of neon atoms.

Added by Derek T.

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