Average Atomic Mass calculation:
● (Mx = A1 M1 + A2 M2 + A3 M3 + (blank) )
● Where mx is the average atomic mass of element x.
● Which has isotopes with masses m1, m2, m3, “x “.
● The natural abundances of which are expressed in decimal form. A1, a2,
a3, “x“
Analyze
● I have to compare the two isotopes and their weight.
● Lighter isotope is more abundant than the average atomic mass will be
less than the average if both isotopes were equally abundant.
● If boron -10 and boron -11 average mass would be 10.5. Since the average
is closer to 11 than it is to 10. Heavier isotopes are more abundant.
Mole
● Cobalt (II) iodine hexahydrate (col2 - 6H2O)
CoI2 x 6H2O
1 Co + 2 I + 12 H + 6 Oxy
1 (58.93) + 2 (120.90)+ 12 (1.008) 6(15.99)
58.93 + 253.8 + 12.096 + 12.096 + 95.94 = 420.8 amu
● How many moles in 400g of carbon?
- C = 12.001
400 / 12.001 = 33.0 g/mol
● Determines the moles of Na3AlF6 provided by 3.25
1000g = kg
Na3AlO2 : Na3AlF6
3:1 Determine the kilograms of NaAlO2 needed to produce 15.5 mol Na3AlF6
3810kg is the same as 3.81 kg NaAlo2