How much electric charge is needed to produce 1.000kg of Na metal from the Na+ ions in NaCl?

You need one electron per atom. How many atoms are present in 1kg of Na? Use avagradros number.

To change to coulombs, remember that 1 electron= 1.6E-19C

To find out how much electric charge is needed to produce 1.000kg of Na metal from the Na+ ions in NaCl, we need to calculate the number of atoms in 1kg of Na using Avogadro's number and then multiply it by the charge of one electron.

Step 1: Find the molar mass of Na.
The molar mass of Na is 22.99 g/mol.

Step 2: Convert 1kg of Na to grams.
Since 1kg = 1000g, we have 1000g of Na.

Step 3: Convert grams of Na to moles.
Using the molar mass of Na (22.99g/mol), we can calculate the moles of Na as follows:
moles = mass in grams / molar mass = 1000g / 22.99g/mol.

Step 4: Calculate the number of atoms using Avogadro's number.
Avogadro's number is approximately 6.022 × 10^23 atoms/mol. Multiply the mol of Na by Avogadro's number:
number of atoms = moles of Na * Avogadro's number.

Step 5: Multiply the number of atoms by the charge of one electron.
Since you need one electron per atom, multiply the number of atoms by the charge of one electron to get the total electric charge:
total charge = number of atoms * (1.6 × 10^-19 C).

By following these steps, you will be able to calculate the amount of electric charge needed to produce 1.000kg of Na metal from the Na+ ions in NaCl.