The mass of an individual atom of calcium is 40.08 amu. How many atoms would weigh a total of 15.46 g of this element if the mass of 1 amu is 1.6605x10-24 g?

40.08 amu/atom x 1.6605E-24g/amu x # atoms = 15.46g.

Solve for # atoms.

To solve this problem, we need to use the given information and convert the mass of calcium to the number of atoms.

First, let's start by converting the mass of one atom of calcium from amu to grams. We use the conversion factor given: 1 amu = 1.6605x10^(-24) g.

Mass of one atom of calcium = 40.08 amu x (1.6605x10^(-24) g/1 amu)
= 40.08 x 1.6605x10^(-24) g
= 6.6508x10^(-23) g

Next, we can calculate the number of atoms of calcium that would weigh a total of 15.46 g:

Number of atoms = Total mass / Mass of one atom

Number of atoms = 15.46 g / (6.6508x10^(-23) g)

Since dividing by a number in scientific notation is challenging, let's convert the divisor to decimal form:

6.6508x10^(-23) g = 0.000000000000000000000066508 g

Now we can calculate the number of atoms:

Number of atoms = 15.46 g / 0.000000000000000000000066508 g

Using a calculator, the result is approximately:

Number of atoms ≈ 2.32494x10^23

Therefore, a total mass of 15.46 g of calcium would contain approximately 2.32494x10^23 atoms.