Home
Class 11
CHEMISTRY
Average atomic mass of magnesium is 24.3...

Average atomic mass of magnesium is `24.31`amu. This magnesium is composed of 79 mole % of `24mg` and remaining 21 mole % of `25mg and 25mg`. Calculate mole % of `26mg`.

Promotional Banner

Similar Questions

Explore conceptually related problems

Average atomic mass of magnesium is 24.31amu. This magnesium is composed of 79 mole % of 24 Mg and remaining 21 mole % of 25Mg and 26 Mg. Calculate mole % of 26 Mg.

Average atomic mass of magnesium is 24.31 amu. This magnesium is composed of 79 mole % of .^(24)Mg and remaining 21 mol % of .^(25)Mg and .^(26)Mg . Calculate mole % of .^(26)Mg .

Average atomic mass of magnesium is 24.31 amu. This magnesium is composed of 79 mole % of .^(24)Mg and reamainig 21 mol % of .^(25)Mg and .^(26)Mg . Calculate mole % of .^(26)Mg .

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 "_12^24Mg (23.98504u), "_12^25Mg (24.98584u) and "_12^26Mg (25.98259u). The natural abundance of "_12^24Mg is 78.99% by mass. Calculate the abundances of other two isotopes.

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 sotopes and their masses are '' - 12^24 Mg (23.98504 u), ''_12^25 12Mg(24.98584 u) and "_12^26 Mg (25.98259 u) . The natural abundance of ''_12^24Mg is 78.99% by mass. Calculate the abundances of other two isotopes.

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 ._12Mg^(24) (23.98504u) , ._(12)Mg^(25) (24.98584) and ._12Mg^(26) (25.98259 u) . The natural abundance of ._12Mg^(24) is 78.99% by mass. Calculate the abundances of the other two isotopes.

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)Mg (23.98504u), ""_(12)^(25)Mg (24.98584u) and ""_(12)^(26)Mg (25.98259u) . The natural abundance of ""_(12)^(24)Mg is 78.99% by mass. Calculate the abundances of other two isotopes.