energy required for ionisation of 0.02 gram atom of magnesium is x Kj .the amount of energy required to ionise 1 atom of magnesium is
Hey there!
Energy required for 0.02 gm of Mg --------->
xkJ
Energy required for 1gm of Mg ------------->
x/0.02 kJ
We know that, 1 atom = 6.022 × 10²³ gm
(6.022 × 10 ²³ is known as Avagadro Number and is donated by NA)
So,
Energy required for NA -----------> x/0.02*NA kJ
Now, let's convert kJ into J
We know that, 1kJ = 1000 J
So, the final answer is,
x*10³/0.02NA J
Hope you got it!
Have a good day!
How many atom in 20 million O2 molecule?
To determine the amount of energy required to ionize one atom of magnesium, we can use the given information that the energy required for ionizing 0.02 gram atom of magnesium is x KJ.
1. First, we need to convert the given mass of magnesium (0.02 gram atom) to the number of moles. We can do this using the molar mass of magnesium.
The molar mass of magnesium (Mg) is approximately 24.31 grams/mol.
Using the formula: Moles = Mass / Molar mass, we can calculate the number of moles of magnesium.
Number of moles = 0.02 grams / 24.31 grams/mol
2. Once we have the number of moles of magnesium, we can use Avogadro's number to determine the number of atoms.
Avogadro's number (Na) is approximately 6.022 x 10^23 atoms/mol.
Number of atoms = Number of moles x Avogadro's number
3. Now that we have the number of atoms, we can find the energy required to ionize one atom.
Energy required to ionize one atom = Energy required to ionize 0.02 gram atom / Number of atoms
Therefore, the amount of energy required to ionize one atom of magnesium is x KJ divided by the number of atoms calculated in step 2.