OK I just need help with two final problems that I am stuck on:

Question

The problem states the calcium carbonate in limestone reacts with HCl to produce a calcium chloride solution and carbon dioxide gas
CaCO3(s)+2HCl(aq)-->CaCl2(aq)+H2O(l)+CO2(g)

1)Find how many moles of CO2 form when 12.5mL of 3.00 M HCl react?

2)What is the molarity of a HCl solution if the reaction of 205 mL of the HCl sloution with excess CaCO3 produces 13.5 L of CO2 gas at 725 mmHg and 18 degrees C?

Answer 1

Just two stoichiometry problems.
1. Write equation and balance it. Done.
2. Convert 12.5 mL of 3.00 M HCl to moles. moles = M x L.
3. Using the coefficients in the balanced equation, convert moles HCl to moles CO2.

#2. Use PV = nRT to solve for n = number of moles CO2.
Convert moles CO2 to moles HCl.
M HCl = molew HCl/L HCl.

Answer 2

molccffvb

Answer 3

1 2 3

Answer 4

you're guys' answers are dogshit