A 1.0 mL sample of seawater is determined to contain 9.0×10-14 moles of dissolved gold.
How many atoms of gold are in that volume of seawater?
To calculate the number of atoms of gold in the given volume of seawater, we can use Avogadro's number, which states that 1 mole of any substance contains 6.022 × 10^23 particles (atoms, molecules, etc.).
First, we need to find the number of moles of gold in the given volume of seawater:
Moles of gold = 9.0 × 10^-14 mol
Since we know the number of moles, we can use Avogadro's number to calculate the number of atoms:
Number of atoms = Moles of gold × Avogadro's number
= 9.0 × 10^-14 mol × 6.022 × 10^23 atoms/mol
Calculating this, we get:
Number of atoms = 5.42 × 10^10 atoms
Therefore, there are approximately 5.42 × 10^10 atoms of gold in 1.0 mL of seawater.
To calculate the number of atoms of gold in a given volume of seawater, you need to use Avogadro's constant and the molar mass of gold. Here's how you can do it:
1. Start with the number of moles of gold in the sample: 9.0×10^(-14) moles.
2. Use Avogadro's constant, which is approximately 6.022×10^(23) atoms/mol, to convert moles to atoms. Multiply the number of moles by Avogadro's constant:
Number of atoms = (9.0×10^(-14) moles) × (6.022×10^(23) atoms/mol)
3. Perform the calculation to find the number of atoms:
Number of atoms = 5.42×10^(10) atoms
Therefore, there are approximately 5.42×10^(10) atoms of gold in the given volume of seawater.