how many moles of gold are there in 1.00 L of seawater if there are 1.50^17 atoms of gold in the sample?
To determine the number of moles of gold in 1.00 L of seawater, we need to convert the given number of atoms of gold into moles.
First, we need to know the Avogadro's number, which is approximately 6.022 × 10^23 atoms/mole.
Now, let's calculate the number of moles of gold:
Number of moles of gold = Number of atoms of gold / Avogadro's number
= 1.50 × 10^17 atoms / 6.022 × 10^23 atoms/mole
Dividing these values, we get:
Number of moles of gold = 2.49 × 10^-7 moles
Therefore, there are approximately 2.49 × 10^-7 moles of gold in 1.00 L of seawater.
To find the number of moles of gold in 1.00 L of seawater, we need to use Avogadro's number.
1 mole of any substance contains 6.022 × 10^23 particles (atoms, molecules, or ions). In this case, we are given the number of atoms of gold.
First, let's calculate the number of moles using Avogadro's number:
Number of moles = Number of atoms / Avogadro's number
Number of moles = 1.50 × 10^17 / 6.022 × 10^23
To perform this calculation, divide 1.50 × 10^17 by 6.022 × 10^23:
Number of moles = 2.49 × 10^-7 moles
Therefore, there are approximately 2.49 × 10^-7 moles of gold in 1.00 L of seawater.
Is 1.00 L the sample?
mols Au = 1.50E17/6.02E23 = ?