Balanced equation: 2HCL+CaCO2>CaCl2+CO2+H2O
what volume of 6.00 M HCL is needed to completely react with .750 moles of CaCO3
To determine the volume of 6.00 M HCl needed to completely react with 0.750 moles of CaCO3, we can use the balanced equation as a conversion factor.
First, let's calculate the number of moles of HCl required. From the balanced equation, we can see that the stoichiometric ratio between HCl and CaCO3 is 2:1. This means that for every 2 moles of HCl, 1 mole of CaCO3 is required.
So, the number of moles of HCl needed can be calculated as follows:
0.750 moles CaCO3 x (2 moles HCl / 1 mole CaCO3) = 1.50 moles HCl
Now, we can use the definition of molarity to convert moles to volume. The formula for molarity is:
Molarity (M) = moles of solute / volume of solution (in liters)
We rearrange the formula to solve for volume:
Volume of solution (in liters) = moles of solute / Molarity
Here, we have the molarity (6.00 M) and the number of moles of HCl (1.50 moles) needed. Substitute these values into the formula:
Volume of HCl = 1.50 moles HCl / 6.00 M HCl
Volume of HCl = 0.25 liters
Therefore, 0.25 liters (or 250 mL) of 6.00 M HCl is needed to completely react with 0.750 moles of CaCO3.