Question

Calculate the volume of CO2, measured at 19°C and 720mmHg pressure, which would beobtained by the action of excess HCl on 10.0g of Calcium trioxocarbonate (IV).​

Answer 1

To calculate the volume of CO2 obtained, first convert the mass of CaCO3 to moles, then determine the moles of CO2 produced using the balanced equation. Finally, use the ideal gas law to calculate the volume of CO2 at the given temperature and pressure.

Step-by-step explanation:

To calculate the volume of CO2 obtained in this reaction, we need to convert the mass of calcium trioxocarbonate (IV) (CaCO3) to moles using its molar mass. Then, using the balanced chemical equation 2HCl + CaCO3 → CaCl2 + CO2 + H2O, we can determine the moles of CO2 produced. Finally, we can use the ideal gas law, PV=nRT, to calculate the volume of CO2 at the given temperature and pressure.

First, calculate the moles of CaCO3: moles = mass / molar mass = 10.0g / 100.09 g/mol = 0.0999 mol.

From the balanced equation, we can see that 1 mole of CaCO3 produces 1 mole of CO2. Therefore, the moles of CO2 produced = 0.0999 mol.

Using the ideal gas law, we can calculate the volume of CO2: V = (nRT) / P = (0.0999 mol)(0.0821 L·atm/mol·K)(19°C + 273.15 K) / (720 mmHg)(1 atm/760 mmHg) = 0.246 L.