Data:
P = 1 atm
V = 5.20 L
n = ?
R = 0.082 for pressures in atmosphere (atm)
T = 136ºC
The temperature to be used in the equation will always be in Kelvim (K), so if it is in degrees Celsius (° C) it is necessary to convert. To do this simply add the value 273.
TK = TºC + 273
TK = 136 + 273
TK = 409
Formula: (General Equation of Perfect Gases)
PV = nRT
15.20 = n0.082409
5.20 = 33.538n
33.538n = 5.20
\(n = \frac{5.20}{33.538}\)
\(\boxed{n \approx 0.15mol}\) of nitrogen molecules
Note: One mole is the amount of matter in a material system containing \(6,02*10^{23}\) particles (elemental entities).
Therefore:
Number atoms in 1 mol of molecules of N2 = 6.0210²³ 2 = 12.0410²³
1mol ---------------- 12,0410²³
0.15 mol ---------------- x
x = 0.15 12,0410²³
x ≈ 1.8*10²³ atoms in 1 mole of N2 molecules.
