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:**

Showing posts with label **SOME BASIC CONCEPT OF CHEMISTRY**. Show all posts

Showing posts with label **SOME BASIC CONCEPT OF CHEMISTRY**. Show all posts

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

** 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.

Illustrative Examples:

Answer Key: 30.33 %

Answer Key: 25

Answer key : 7.092×10^7

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