We know that for gas:
Pressure fraction = Mole fraction= Volume fraction
Pressure % = Mole % = Volume %
Consider mixture of two different gases (A) and (B) and their moles nA
and nB
Illustrated Examples:We know that for gas:
Pressure fraction = Mole fraction= Volume fraction
Pressure % = Mole % = Volume %
Consider mixture of two different gases (A) and (B) and their moles nA
and nB
Illustrated Examples:Answer Key: VD :2.7
Answer Key: 0.2 Mole
Answer Key: (1) 20% and 80% (2) 11.1%
Answer Key: ( N2O4)
Answer Key: (1) 25 gm (2) 40 %
Answer Key: Mav = 23.8 amu , % by mass of Oxygen = 22.3 % and % by mass of Nitrogen is 77.7 %
Answer Key: The average atomic mass of silicon is 28.1 amu
Answer Key: Ag (107) 25% and Ag (109) 75%
Answer Key: A= 10
Answer Key: 1.000199 amu
SOLUTION: Molar mass of Ar
= 35.96755 × 0.071 + 37.96272 × 0.163 + 39.96924 × 0.766
= 39.352 g mol−1
Elements are found in different isotopic forms (atoms of same elements having different atomic mass), so the atomic mass of any element is the average of all the isotopic mass within a given sample.
(A) If an elements exists in two isotopes having atomic masses ‘M1’ and ‘M2’ in the ratio X: Y, then
or
(B) If an elements exists in two isotopes having atomic masses ‘M1’ and ‘M2’ and their abundant percentage (%) are X % and Y % then
Since the atomic mass is a ratio, it has no units and is expressed in amu.