What amount of energy is required to completely ionize 21.5 grams of carbon atoms in the gas phase (C(g)) if the ionization energy of C(g) is 1086 kJ/mole?

Answer in units of J

Ionize it to what? one electron?

21.5/12 = mols C
1086 kJ/mol x ?mol = ?

To find the amount of energy required to completely ionize a given mass of carbon atoms, we need to follow these steps:

Step 1: Determine the molar mass of carbon atoms.
The molar mass of carbon (C) is 12 g/mol.

Step 2: Convert the given mass of carbon atoms to moles.
To convert grams to moles, we divide the given mass by the molar mass:
Number of moles of carbon = mass of carbon / molar mass of carbon
= 21.5 g / 12 g/mol
ā‰ˆ 1.792 moles

Step 3: Calculate the energy required to ionize the given moles of carbon atoms.
The ionization energy of carbon is given as 1086 kJ/mol.
To convert kilojoules to joules, we multiply the value by 1000:
Ionization energy of carbon = 1086 kJ/mol * 1000 J/kJ
= 1,086,000 J/mol

Now, to find the energy required to ionize the given moles of carbon atoms, we multiply the ionization energy by the number of moles:
Energy required to ionize carbon atoms = Ionization energy of carbon * moles of carbon
= 1,086,000 J/mol * 1.792 moles
ā‰ˆ 1,948,112 J

Therefore, approximately 1,948,112 joules of energy is required to completely ionize 21.5 grams of carbon atoms in the gas phase (C(g)).