You have a 12.01 g sample of carbon. The average mass of a carbon atoms is 1.994 x 1023 g. How many carbon atoms are in the sample?
I don't believe the average mass of a C atom is anywhere near 1.994E23 g!
To find the number of carbon atoms in the sample, we need to use the given information about the mass of the carbon atom and the mass of the sample of carbon.
First, let's determine the number of moles of carbon in the sample:
1. Calculate the moles of carbon in the sample by dividing the mass of the sample by the average mass of a carbon atom:
Moles = Mass of the sample / Average mass of a carbon atom
In this case:
Mass of the sample = 12.01 g
Average mass of a carbon atom = 1.994 x 10^23 g
Moles = 12.01 g / (1.994 x 10^23 g)
Now we can convert the moles of carbon to the number of carbon atoms:
2. Use Avogadro's Number, which states that 1 mole of any substance contains 6.022 x 10^23 particles (atoms, molecules, etc.).
Number of atoms = Moles of carbon * Avogadro's Number
Plug in the value of Avogadro's Number, 6.022 x 10^23 particles, and the moles calculated in step 1 to get the final answer.
Therefore, the number of carbon atoms in the given 12.01 g sample of carbon would be:
Number of atoms = (12.01 g / (1.994 x 10^23 g)) * (6.022 x 10^23 atoms)
Simplifying the calculation will give us the exact number of carbon atoms in the sample.