Common brass is a copper and zinc alloy containing 37.0% zinc by mass and having a density of 8.48 . A fitting composed of common brass has a total volume of 114.5 .How many atoms of copper does the fitting contain?

density of 8.48 g/cm3

volume of 114.5 cm3
of brass

114.5 cc volume.

8.48 g/cc = density.
mass = volume x density = 114.5 cc x 8.48 g/cc = ??grams.

37% of that is Zn; therefore, (100-37 = %Cu)
?? grams x 0.63 = g Cu.
Convert that to moles (moles = grams/molar mass), then to atoms remembering that 1 mole of atoms contains 6.022 x 10^23 atoms of Cu.

To find the number of atoms of copper in the fitting, we need the mass of copper present in the fitting and the molar mass of copper.

Let's break it down step by step:

1. Calculate the mass of copper in the fitting:
We know that the fitting is made of common brass, which contains 37.0% zinc. Therefore, the percentage of copper in the alloy is 100% - 37.0% = 63.0%.

Mass of copper = 63.0% of total mass of the fitting

To find the mass of copper, we multiply the total mass of the fitting by 63.0%:
Mass of copper = 0.63 * Total mass of the fitting

2. Determine the molar mass of copper:
The molar mass of copper (Cu) can be found on the periodic table. It is approximately 63.55 g/mol.

3. Calculate the number of moles of copper:
Number of moles of copper = Mass of copper / Molar mass of copper

4. Use Avogadro's number to determine the number of atoms:
One mole of any substance contains 6.022 x 10^23 atoms (Avogadro's number).

Number of atoms of copper = Number of moles of copper * Avogadro's number

Let's put the values into the equations:

1. Mass of copper = 0.63 * Total mass of the fitting
2. Molar mass of copper = 63.55 g/mol
3. Number of moles of copper = Mass of copper / Molar mass of copper
4. Number of atoms of copper = Number of moles of copper * Avogadro's number

8.48 WHAT?

114.5 WHAT?