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  • Compute the difference in masses of one mole each of aluminum atoms and one mole of its ions \left ( Mass \: \: of\: \: an\: \: electron\: \: is\: \: 9.1 \times 10^{-28} g \right ) Which one is heavier

Compute the difference in masses of one mole each of aluminum atoms and one mole of its ions.

\left ( Mass \: \: of\: \: an\: \: electron\: \: is\: \: 9.1 \times 10^{-28} g \right ) Which one is heavier?

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best_answer

Ionization of Al atom occurs as  

Al\rightarrow Al^{3+}+3e^-

Therefore, Al^{3+} ion is formed from Al atom by loss of 3 electrons. Difference in mass of 1 mole of Al atoms and 1 mole of Al^{3+} ions

= mass\: \: of \: \: 3 \times 6.022 \times 10^{23} electrons

= (3 \times 6.022 \times 10^{23}) \times (9.1 \times 10^{-28} g)

(as \: \: mass\: \: of\: \: an \: \: electron = 9.1 \times 10^{-28} g)

=164.4 \times 10^{-5}g=1.644 \times 10^{-3}g

1 mole of Al atoms is heavier than 1 mole of  Al^{3+} ions.

It is because 1 mole of Al atom have e^-= 13\times 6.022 \times 10^{23 } electrons and  1 mole of Al ion have 

e=10\times 6.022 \times 10^{23 } electrons 

 

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infoexpert26

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