(C) The average atomic mass is calculated using the formula: $Avg. \text{ atomic mass} = \frac{m_1 x_1 + m_2 x_2 + m_3 x_3}{x_1 + x_2 + x_3}$ Substitu

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(C) The average atomic mass is calculated using the formula: $Avg. \text{ atomic mass} = \frac{m_1 x_1 + m_2 x_2 + m_3 x_3}{x_1 + x_2 + x_3}$ Substituting the given values: $Avg. \text{ atomic mass} = \frac{11 \times 80 + 12 \times 15 + 13 \times 5}{80 + 15 + 5}$ $= \frac{880 + 180 + 65}{100} = \frac{1125}{100} = 11.25$

Class 11 Chemistry Some Basic Concepts of Chemistry Atomic, Molecular and Equivalent masses

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An element has three isotopes and their isotopic weights are $11, 12, 13$ units,and their percentage of occurrence in nature is $80 \%, 15 \%, 5 \%$ respectively. Then the average atomic weight of the element will be $:-$

A
$11.20$
B
$11.2$
C
$11.25$
D
$112.5$

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Class 11

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Some Basic Concepts of Chemistry

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Atomic, Molecular and Equivalent masses

Naturally occurring boron has $20\%$ $_5B^{10}$ and $80\%$ $_5B^{11}$. The average atomic weight of boron is

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Sulphur forms the chlorides $S_2Cl_2$ and $SCl_2$. The equivalent mass of sulphur in $SCl_2$ is $...$ $g/mol$.

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If $1.2 \, g$ of a metal displaces $1.12 \, L$ of hydrogen at $STP$,the equivalent weight of the metal would be:

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When the weights of two elements combine with each other,their ratio is the ratio of their ......

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If $M_1$ and $M_2$ are the molecular weights of $Al(OH)_3$ and $H_3PO_3$ respectively,find their equivalent weights in the following reaction:
$Al(OH)_3 + 2H_3PO_3 \to Al(OH)(H_2PO_3)_2 + 2H_2O$

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An element has three isotopes and their isotopic weights are $11, 12, 13$ units,and their percentage of occurrence in nature is $80 \%, 15 \%, 5 \%$ respectively. Then the average atomic weight of the element will be $:-$

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Naturally occurring boron has $20\%$ $_5B^{10}$ and $80\%$ $_5B^{11}$. The average atomic weight of boron is

Sulphur forms the chlorides $S_2Cl_2$ and $SCl_2$. The equivalent mass of sulphur in $SCl_2$ is $...$ $g/mol$.

If $1.2 \, g$ of a metal displaces $1.12 \, L$ of hydrogen at $STP$,the equivalent weight of the metal would be:

When the weights of two elements combine with each other,their ratio is the ratio of their ......

If $M_1$ and $M_2$ are the molecular weights of $Al(OH)_3$ and $H_3PO_3$ respectively,find their equivalent weights in the following reaction:$Al(OH)_3 + 2H_3PO_3 \to Al(OH)(H_2PO_3)_2 + 2H_2O$

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If $M_1$ and $M_2$ are the molecular weights of $Al(OH)_3$ and $H_3PO_3$ respectively,find their equivalent weights in the following reaction:
$Al(OH)_3 + 2H_3PO_3 \to Al(OH)(H_2PO_3)_2 + 2H_2O$