The balanced equation shows how sodium chloride reacts with silver nitrate to form sodium nitrate and silver chloride. NaCl + AgNO3 NaNO3 + AgCl If 4.00 g of NaCl react with 10.00 g of AgNO3, what is the excess reactant

The excess reactant is the NaCl.

Explanation:

NaCl(aq) + AgNO3 (aq) → NaNO₃(aq) + AgCl (s) ↓

This is a precipitation reaction.

We need to convert the mass of each reactant to moles:

4 g / 58.45 g/mol = 0.068 moles of NaCl

10 g / 169.87 g/mol = 0.059 moles of nitrate.

As stoichiometry is 1 by 1, 1 mol of chloride will react with 1 mol of nitrate.

If I have 0.059 moles of nitrate, I will need the same amount of chloride and I have 0.068 moles. I still have chloride, therefore the excess reactant is the NaCl.

0.068 mol - 0.059 mol = 0.009 moles are the moles of NaCl that remains after the reaction is complete

we can conclude that the melting point of table salt is above room temperature (it's actually 801 deg c). the melting point of mercury must be below room temperature (- 39 deg c).