Chemistry help plzzz

Question

How many moles of BaCl2 form when 1.50 mol of HCL reacts with excess barium hydroxide in a aqueous solution

Answer 1

Step 1: Write a balanced chemical reaction equation

2HCL + Ba(OH)₂ → BaCl₂ + 2H₂O

Explanation:

First, make sure you get all the compounds in the correct places. The problem states the reactants (left side of the arrow) are barium hydroxide and HCl. We need to figure out how to write the chemical compound formula of the barium hydroxide. We look up Barium on the Periodic Table and see it has a +2 charge. We look up hydroxide and see it is OH and see it has a -1 charge so we need 2 of them to electrically balance with the +2 Barium. Then, using the HCL and Ba(OH)₂, we write out the equation, and we see there are only O's and H's left on the right side (products) after we write the BaCl₂ in as a product. We realize that H₂O is not only a combination of H's and O's but is also a reasonable product in an acid/base reaction. So we write the products as BaCl₂ and H₂O. Then we balance the equation by adding a couple of 2's.

Step 2: Use the molar ratios to get the answer

The chemical reaction equation is an equation in moles. It says that for every 2 moles of HCl, there is 1 mole of BaCl₂ produced. So we set up a conversion to calculate the moles of BaCl₂ produced:

Notice that we have moles of HCl on both top and bottom that cancel out and leave us with moles of BaCl₂ which is what we want. Then we just do the math (divide 1.5 by 2) to get 0.75 moles of BaCl₂. Finally, we ust the correct number of sig figs. The "givens" use 3 sig figs (1.50) so we use 3 sig figs in our answer:

There are 0.750 moles of of BaCl₂ produced.

Answer 2