Water standing in the open at 29.2°c evaporates because of the escape of some of the surface molecules. the heat of vaporization (548 cal/g) is approximately equal to εn, where ε is the average energy of the escaping molecules and n is the number of molecules per gram.
(a) find ε.
(b) what is the ratio of ε to the average kinetic energy of h2o molecules, assuming the latter is related to temperature in the same way as it is for gases?

a) ε = 6.86x J

b) ε/Kavg = 10.98

Explanation:

a) The heat of evaporation (Lv) is

Lv = εn

ε = Lv/n

n is the number of molecules in a gram of the substance. The molar mass of water (H2O) is 2x1 g of H + 16 g of O = 18 g/mol.

By the Avogadros' number(NA), we know that 1 mol = 6.02x molecules, so n will be:

n = NA/ molar mass

n =

n = 3.34x molecules/g

So,

ε =

ε = 1.64x cal

As 1 cal = 4.18 J, ε = 6.86x J

b) For ideal gases, the average of the kinetic energy (the internal energy of the molecules) is given by :

Kavg = kT

Where Kavg is the average of the kinetic energy, k is the Boltzmann's constant and T is the temperature in Kelvin.

Knowing that k = 1.38x J/K and T = 29.2ºC + 273 = 302.2 K

Kavg = x1.38xx302.2

Kavg = 6.25x J

So the ratio of ε to the average kinetic energy of H2O molecules is

ε/Kavg =

ε/Kavg = 10.98

is has three carbons, so the answer is propylamine.

meth-

eth-

prop-

but-

pent-

hex-

hept-

oct-

non-

explanation:

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%