Given, Lv = 540\(\frac{kcal}{Kg}\)
= 540 × 103 × 4.2 J/Kg
(a) Such that, 1kg of water requires energy for evaporation = Lv k cal
∴ MA kg of water requires MALvk cal
Since there are NA molecules to evaporates is
\(u=\frac{M_AL_v}{N_A}J\) [Here, NA = 6 × 1026 = Avogadro number]
= \(\frac{18×540×4.2×10^3}{6×10^{26}}\)
= 90 × 18 × 4.2 × 10-23 J
= 6.8 × 10-20 J
(b) Let us consider the water molecules to be points at a distance d from each other.
Volume of NA molecules = \(\frac{M_A}{ρ_w}l\)
Thus, the volume around one molecule is \(\frac{M_A}{N_Aρ_w}l\)
The volume around one molecule is d3 = (\(\frac{M_A}{N_Aρ_w}\))
∴ d = \((\frac{M_A}{N_Aρ_w})^\frac{1}{3}\) = \((\frac{18}{6×10^{26}×10^3})^\frac{1}{3}\)
= (3 × 10−30)\(\frac{1}{3}\) m ≃ 3.1 × 10−10 m
(c) 1 kg of vapour occupies = 1601 × 10-3 m3
∴ 18 kg of vapour occupies = 18 × 1601 × 10-3 m3
or 6 × 1026 molecules occupies = 18 × 1601 × 10-3 m3
∴ 1 molecule occupies = \(\frac{18×1601×10^3}{6×10^{26}}m^3\)
If d1 is the inter molecular distance.
Then
\(d^3_1\) = (3 × 1601 × 10-29) m3
∴ d1 = (30 × 1601)\(\frac{1}{3}\) × 10-10 m
= 36.3 × 10-10 m
(d) To change the distance from d to d1,
Work done = F(d1 − d)
Work done = energy required to evaporate 1 molecule
Or F = \(\frac{6.8×10^{−20}}{d_1−d}\)
= \(\frac{6.8×10^{−20}}{ (36.3−3.1)×10^{−10}}\)
= 0.2048 × 10−10 N
(e) Surface Tension = \(\frac{F}{d}\)
= \(\frac{2.05×10^{−20}}{3.1×10^{−10}}\)
= 6.6 × 10-2 Nm-1