What amount of energy is required to com-

pletely ionize 26.9 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

To find the amount of energy required to completely ionize 26.9 grams of carbon atoms (C) in the gas phase (C(g)), we need to first calculate the number of moles of carbon atoms present. Then, we can use the ionization energy to calculate the total energy.

Step 1: Calculate the number of moles of carbon atoms:
First, we need to determine the molar mass of carbon (C). The atomic mass of carbon is approximately 12.01 g/mol.

Number of moles = Mass / Molar mass
Number of moles = 26.9 g / 12.01 g/mol
Number of moles ā‰ˆ 2.24 mol

Step 2: Calculate the total energy required:
Now that we know the number of moles of carbon atoms, we can calculate the total energy required.

Total energy = Number of moles * Ionization energy
Total energy = 2.24 mol * 1086 kJ/mol

To convert kJ to J, we need to multiply by 1000:
Total energy = 2.24 mol * 1086 kJ/mol * 1000 J/1 kJ

Now, let's calculate the result:

Total energy = 2.24 * 1086 * 1000 J
Total energy ā‰ˆ 2,418,240 J

Therefore, the amount of energy required to completely ionize 26.9 grams of carbon atoms in the gas phase is approximately 2,418,240 Joules.

1086 kJ/mol x # mol = ?kJ.

How many mols do you have? That is
mols = grams/atomic mass.