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

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?

you're guys' answers are dogshit

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.

Sure, I can help you with those two problems!

1) To find the moles of CO2 formed, we need to use the given volume of HCl and its concentration.
First, we need to convert the volume of HCl from milliliters (mL) to liters (L). There are 1000 mL in 1 L, so:

12.5 mL * (1 L / 1000 mL) = 0.0125 L

Next, we can use the volume and concentration of HCl to calculate the number of moles of HCl we have:

moles of HCl = volume of HCl (in Liters) * concentration of HCl (in moles/L)
= 0.0125 L * 3.00 moles/L

Now, looking at the balanced equation, we see that the stoichiometry of the reaction is 2 moles of HCl to 1 mole of CO2. So, to calculate the moles of CO2 formed, we can use the mole ratio:

moles of CO2 = (moles of HCl) * (1 mole of CO2 / 2 moles of HCl)

Now you can plug in the value for moles of HCl and calculate the moles of CO2 formed.

2) To find the molarity of the HCl solution, we can use the given volume of the HCl solution that reacts and the volume of CO2 gas produced.
First, convert the volume of the HCl solution from milliliters (mL) to liters (L):

205 mL * (1 L / 1000 mL) = 0.205 L

Next, convert the volume of CO2 gas produced from liters (L) to moles (mol) using the ideal gas law equation:

moles of CO2 = (volume of CO2 gas in L) * (pressure in atm) / (gas constant R) * (temperature in Kelvin)

Here, you are given the volume of CO2 gas (13.5 L), the pressure (725 mmHg), and the temperature (18 degrees C). To use the ideal gas law, we need to convert the pressure to atm and the temperature to Kelvin:

pressure in atm = 725 mmHg * (1 atm / 760 mmHg)
temperature in Kelvin = 18 degrees C + 273.15

Now, you can calculate the moles of CO2 gas produced.

Since the reaction is with excess CaCO3, all the moles of CO2 produced come from the reaction with HCl. Therefore, the moles of CO2 produced are equal to the moles of HCl reacted. Now you can use the moles of HCl (which is the same as moles of CO2) and the volume of HCl solution (in Liters) to calculate the molarity of the HCl solution:

Molarity (M) = moles of HCl / volume of HCl solution (in L)

I hope this helps!

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