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Physics Part-II

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In a periodic table the average atomic mass of magnesium is gi

Physics Part-II

Class 12

NCERT

Chapter 1: Ray Optics and Optical Instruments

41 questions

Chapter 2: Wave Optics

30 questions

Chapter 3: Dual Nature of Radiation and Matter

44 questions

Chapter 4: Atoms

23 questions

Chapter 5: Nuclei

38 questions

For the

β^{+}

(positron) emission from a nucleus, there is another competing process known as electron capture (electron from an inner orbit, say, the K shell, is captured by the nucleus and a neutrino is emitted).

e^{+} +_{Z}^{A} X \to_{Z - 1}^{A} Y + v

Show that if

β^{+}

emission is energetically allowed, electron capture is necessarily allowed but not vice versa.

In a periodic table the average atomic mass of magnesium is given as 24.312 u. The average value is based on their relative natural abundance on earth. The three isotopes and their masses are

_{12}^{24} M g

(23.98504u),

_{12}^{25} M g

(24.98584u) and

_{12}^{26} M g

(25.98259u). The natural abundance of

_{12}^{24} M g

is 78.99% by mass. Calculate the abundances of other two isotopes.

The neutron separation energy is defined as the energy required to remove a neutron from the nucleus. Obtain the neutron separation energy of the nuclei

_{13}^{27} A l

from the following data:

m (_{13}^{26} A l) = 25.986895 u

m (_{13}^{27} A l) = 26.981541 u

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Chapter 6: Semiconductor Electronics: Materials, Devices and Simple Circuits

25 questions

Question

Easy

Solving time: 4 mins

In a periodic table the average atomic mass of magnesium is given as 24.312 u. The average value is based on their relative natural abundance on earth. The three isotopes and their masses are $_{12}^{24} M g$ (23.98504u), $_{12}^{25} M g$ (24.98584u) and $_{12}^{26} M g$ (25.98259u). The natural abundance of $_{12}^{24} M g$ is 78.99% by mass. Calculate the abundances of other two isotopes.

Name: Video solution 1: [Solved] In a periodic table the average atomic mass of magnesium is given as 24.312 u. The average value is based on their relative natural abundance on earth. The three isotopes and their masses are 1224Mg (23.98504u), 1225Mg (24.98584u) and 1226Mg (25.98259u). The natural abundance of 1224Mg is 78.99% by mass. Calculate the abundances of other two isotopes. - Physics Part-II
Uploaded: 2022-06-15T13:01:26.000Z
Duration: 2 min
Description: Video solution 1: [Solved] In a periodic table the average atomic mass of magnesium is given as 24.312 u. The average value is based on their relative natural abundance on earth. The three isotopes and their masses are 1224Mg (23.98504u), 1225Mg (24.98584u) and 1226Mg (25.98259u). The natural abundance of 1224Mg is 78.99% by mass. Calculate the abundances of other two isotopes. - Physics Part-II

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Updated on: Jun 15, 2022

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Physics Part-II (NCERT)

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In a periodic table the average atomic mass of magnesium is given as 24.312 u. The average value is based on their relative natural abundance on earth. The three isotopes and their masses are

_{12}^{24} M g

(23.98504u),

_{12}^{25} M g

(24.98584u) and

_{12}^{26} M g

(25.98259u). The natural abundance of

_{12}^{24} M g

is 78.99% by mass. Calculate the abundances of other two isotopes.

6 mins ago

Discuss this question LIVE

6 mins ago

Text solutionVerified

Let, the abundance of

_{12} M g^{25}

by mass be x%.

Therefore, abundance of

_{12} M g^{26}

by mass=

(100 - 78.99 - x)

= (21.01 - x)

Now, average atomic mass of Mg is

24.312 = 23.98504 \times \frac{78.99}{100} + 24.98584 \times \frac{x}{100} + 25.98259 \times \frac{21.01 - x}{100}

⟹ x = 9.303

% for

_{12} M g^{25}

(21.01 - x)

= 11.71

% for

_{12} M g^{26}

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Practice more questions from Physics Part-II (NCERT)

For the

β^{+}

e^{+} +_{Z}^{A} X \to_{Z - 1}^{A} Y + v

Show that if

β^{+}

emission is energetically allowed, electron capture is necessarily allowed but not vice versa.

In a periodic table the average atomic mass of magnesium is given as 24.312 u. The average value is based on their relative natural abundance on earth. The three isotopes and their masses are

_{12}^{24} M g

(23.98504u),

_{12}^{25} M g

(24.98584u) and

_{12}^{26} M g

(25.98259u). The natural abundance of

_{12}^{24} M g

is 78.99% by mass. Calculate the abundances of other two isotopes.

The neutron separation energy is defined as the energy required to remove a neutron from the nucleus. Obtain the neutron separation energy of the nuclei

_{13}^{27} A l

from the following data:

m (_{13}^{26} A l) = 25.986895 u

m (_{13}^{27} A l) = 26.981541 u

View all

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Question Text	In a periodic table the average atomic mass of magnesium is given as 24.312 u. The average value is based on their relative natural abundance on earth. The three isotopes and their masses are $_{12}^{24} M g$ (23.98504u), $_{12}^{25} M g$ (24.98584u) and $_{12}^{26} M g$ (25.98259u). The natural abundance of $_{12}^{24} M g$ is 78.99% by mass. Calculate the abundances of other two isotopes.
Updated On	Jun 15, 2022
Topic	Nuclei
Subject	Physics
Class	Class 12
Answer Type	Text solution:1 Video solution: 1
Upvotes	154
Avg. Video Duration	2 min

Text solutionVerified

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