CaCo3 reacts with aq HCl to give CaCl2+CO2. What mass of CaCo3 is required to react completely with 50cm^3 of 0.60M HCl. Calculate volume of CO2 produced at STP.

CaCO3 + 2HCl ==> CaCl2 + H2O + CO2

mols HCl = M x L = ?
Using the coefficients in the balanced equation, convert mols HCl to mols CaCO3.
Now convert mols CaCO3 to grams. grams = mols x molar mass = ?

For part 2. use the coefficients to convert mols HCl to mols CO2. hen volume CO2 = mols x 22.4 L/mol = ? Liters.

To determine the mass of CaCO3 required for the reaction, we need to use stoichiometry. The balanced chemical equation for the reaction is:

CaCO3 + 2HCl → CaCl2 + CO2

From the equation, we can see that 1 mole of CaCO3 reacts with 2 moles of HCl, producing 1 mole of CO2.

Step 1: Calculate the number of moles of HCl using the given volume and concentration:
Number of moles of HCl = (volume in liters) x (concentration in moles per liter)
= 0.050 L x 0.60 mol/L
= 0.030 mol

Step 2: Apply mole ratio to determine the number of moles of CaCO3 required:
From the balanced equation, we know that 1 mole of CaCO3 reacts with 2 moles of HCl.
Therefore, the number of moles of CaCO3 = 0.030 mol HCl x (1 mol CaCO3 / 2 mol HCl) = 0.015 mol CaCO3

Step 3: Calculate the mass of CaCO3 using its molar mass:
Molar mass of CaCO3 = (1 x atomic mass of Ca) + (1 x atomic mass of C) + (3 x atomic mass of O)
= 40.08 g/mol + 12.01 g/mol + (3 x 16.00 g/mol)
= 40.08 g/mol + 12.01 g/mol + 48.00 g/mol
= 100.09 g/mol

Mass of CaCO3 = number of moles x molar mass
= 0.015 mol x 100.09 g/mol
= 1.501 g
= 1.50 g (rounded to two decimal places)

Therefore, 1.50 grams of CaCO3 is required to react completely with 50 cm^3 of 0.60M HCl.

Now, let's calculate the volume of CO2 produced at STP (Standard Temperature and Pressure).
STP conditions are 0 degrees Celsius (273.15 K) and 1 atmosphere (atm) pressure.

Step 1: Calculate the number of moles of CO2 produced:
From the balanced equation, we know that 1 mole of CaCO3 produces 1 mole of CO2.
Therefore, the number of moles of CO2 = 0.015 mol (which we calculated earlier).

Step 2: Apply the ideal gas equation to calculate the volume of CO2 at STP:
PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/(mol·K)), and T is the temperature in Kelvin.

At STP, the pressure (P) is 1 atm and the temperature (T) is 273.15 K.

V = (nRT) / P
= (0.015 mol) x (0.0821 L·atm/(mol·K)) x (273.15 K) / (1 atm)
= 0.3394 L
= 339.4 cm^3 (rounded to two decimal places)

Therefore, the volume of CO2 produced at STP is 339.4 cm^3.