Calculate the mass of NaCl that must be added to completely react with 1.50 L of a 0.150 M AgNO3 solution according to the reaction below: NaCl (aq) + AgNO3 (aq) → AgCl (s) + NaNO3 (aq)

Explanation:

Hello,

In this case, since the reaction is:

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

And it is properly balanced, given 1.50 L of 0.150-M AgNO3, the first step is to compute the moles of reacting silver nitrate as follows given its volume and concentration:

Next, by applying stoihiometry, given the 1:1 mole ratio between silver nitrate and sodium chloride, we compute the mass of NaCl by also using its molar mass (58.45 g/mol):

Regards.

n+h→nh3

we must remember that nitrogen and hydrogen are both diatomic molecules in their standard gas form. this adjusts the equation to

n2+h2→nh3

now we need to adjust coefficients in order to balance the atoms on each side of the equation. currently we have 2 atoms of nitrogen and 2 atoms of hydrogen on the reactant side and 1 atom of nitrogen and 3 atoms of hydrogen on the product side.

we can balance the hydrogens by placing a coefficient of 2 in front of ammonia and a coefficient of 3 in front of the hydrogen.

n2+3h2→2nh3

this gives us 6 hydrogen on each side and coincidentally the nitrogens now equal 2 on each side.