A silver ring contains 0.0134 mmol Ag. How many silver atoms does it contain?
0.0134mol/1000=1.34×10^-5
1.34×10^-5 (6.022×10^23)
=8.07×10^18
To determine the number of silver atoms in the ring, we need to convert the given amount from moles to atoms.
1. First, let's convert the given amount from millimoles (mmol) to moles.
Since 1 mmol = 0.001 mol, we have:
0.0134 mmol Ag = 0.0134 × 0.001 mol Ag = 0.0000134 mol Ag
2. Now, we need to find the Avogadro's number, which represents the number of atoms in one mole of a substance.
Avogadro's number (NA) = 6.022 × 10^23 atoms/mol
3. Finally, we can find the number of silver atoms in the ring by multiplying the amount in moles by Avogadro's number.
Number of silver atoms = 0.0000134 mol Ag × 6.022 × 10^23 atoms/mol
Let's calculate the result:
Number of silver atoms = 8.0748 × 10^19 atoms
Therefore, the silver ring contains approximately 8.0748 × 10^19 silver atoms.
To determine the number of silver atoms in a silver ring, we need to use the Avogadro's number (6.022 x 10^23 atoms per mole) and the number of moles of silver present.
First, convert the given amount of silver from millimoles (mmol) to moles by dividing it by 1000:
0.0134 mmol Ag / 1000 = 0.0000134 mol Ag
Now, we can use Avogadro's number to calculate the number of silver atoms:
0.0000134 mol Ag x (6.022 x 10^23 atoms/mol) = 8.07 x 10^18 silver atoms.
Therefore, the silver ring contains approximately 8.07 x 10^18 silver atoms.