The average atomic mass of molybdenum (Mo) is 95.94 amu. Which of the following isotopes must have the highest percent abundance
1 answer:
Answer:
The two isotopes of Molybdenum have equal natural abundance
Explanation:
= 95.95 amu
x = (95.95 * 2) - 95.94
= 95.96 amu is isotope B, while 95.94amu is isotope A
Using the formula x + (1 - x) = 1
95.96x + 95.94 (1-x) = 95.95
95.96x + 95.94 - 95.94x = 95.95
0.02x = 0.01
x = 0.5
<u>∴ Isotope A and B have equal abundance since 0.5 = 50% abundance.</u>
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Answer:
The answer to your question is 71.22 g
Explanation:
Data
Density = 19.3 g/cm³
Volume = 0.00369
mass = ?
Formula
Density =
Solve for mass
mass = density x volume
Process
1.- Convert volume from liters to cubic centimeters
1 l ---------------- 1000 cm³
0.00369l --------- x
x = (0.00369 x 1000 ) / 1
x = 3.69 cm³
2.- Substitution
mass = 19.3 x 3.69
3.- Simplification and result
mass = 71.22 g