Question

What is the volume of CO2 (acting as an ideal gas) if 64.0 mL of 1.261 M HCl reacts with excess

CaCO3 at 28 °C and 0.987 atm? Show your work and box your answer
2HCl + CaCO3 + H2O + CO2 + CaCl2

Answer 1

1.01 L

Step-by-step explanation:

Step 1: Write the balanced equation

2 HCl + CaCO₃ ⇒ H₂O + CO₂ + CaCl₂

Step 2: Calculate the reacting moles of HCl

64.0 mL (0.0640 L) of 1.261 M (1.261 mol/L) HCl react. The reacting moles are:

0.0640 L × 1.261 mol/L = 0.0807 mol

Step 3: Calculate the moles of CO₂ produced from 0.0807 moles of HCl

The molar ratio of HCl to CO₂ is 2:1. The moles of CO₂ produced are 1/2 × 0.0807 mol = 0.0404 mol.

Step 4: Calculate the volume occupied by 0.0404 moles of CO₂

0.0404 moles of CO₂ are at 28 °C (301 K) and 0.987 atm. We can calculate the volume occupied using the ideal gas equation.

P × V = n × R × T

V = n × R × T / P

V = 0.0404 mol × (0.0821 atm.L/mol.K) × 301 K / 0.987 atm = 1.01 L