Molar Volume of a Gas (Edexcel International AS Chemistry)

Measuring gas volumes

• The volume of gas produced in a reaction can be measured by collecting the gas with a gas syringe or by the displacement of water

Sample method

• For the reaction of hydrochloric acid and sodium carbonate

Na₂CO₃ (s) + 2HCl (aq) → 2NaCl (aq) + H₂O (l) + CO₂ (g)

1. Measure out a fixed volume of hydrochloric acid, e.g. 25.0 cm³, into a conical flask
2. Add a known mass of sodium carbonate, e.g. 0.05 g, to the conical flask
3. Immediately connect the gas syringe delivery tube
4. Allow the reaction to go to completion
5. Record the volume of carbon dioxide produced
6. Repeat the experiment with different masses of sodium carbonate, e.g. 0.10 g, 0.15 g, 0.20 g, 0.25 g... 0.50 g
7. Some assumptions are made about the experiment:
   • The amount of gas lost between adding the sodium carbonate and connecting the delivery tube is negligible
   • The delivery tube set up is airtight so no gas is lost
   • The reaction does go to completion

Sample results

Mass Volume Results Table

• The results are then plotted on to a graph
  • Mass of sodium carbonate on the x-axis and volume or carbon dioxide produced on the y-axis
• Anomalous results are ignored and one straight line (or one smooth curve) of best fit is added

Analysis

• Read off the volume of gas produced for a sensible mass of sodium carbonate, e.g. 0.35 g produces 79.0 cm³ 
  • The mass of sodium carbonate may be specified in an exam question

Na₂CO₃ (s) + 2HCl (aq) → 2NaCl (aq) + H₂O (l) + CO₂ (g)

• From the reaction equation, one mole of sodium carbonate produces one mole of carbon dioxide
• Calculate the molar mass of sodium carbonate 
  • (2 x 23.0) + 12.0 + (3 x 16.0) = 106.0
• Calculate the number of moles of sodium carbonate, using the mass from your graph reading
  • Moles 0.0033 moles
• Convert the volume of carbon dioxide from your graph reading from cm³ to dm³ 
  • = 0.079 dm³
• Calculate the molar volume of gas produced:
  • Molar gas volume 23.93 dm³ 

Application

• This experiment can be used to determine the identity of an unknown metal, M, in a metal carbonate, MCO₃ 
• This process can be applied to thermal decomposition of metal carbonates as well as their reaction with acid

Answer:

Step 1: Find the number of moles of carbon dioxide released using the volume produced at room temperature and pressure:

• • number of moles of CO₂ =
  • n(CO₂) = = 0.009417 mol

Step 2: Find the number of moles of metal carbonate, MCO₃ 

• • One mole of metal carbonate will release one mole of carbon dioxide
  • Number of moles of CO₂ = number of moles of MCO₃ 
  • n(MCO₃) = 0.009417 mol

Step 3: Calculate the molar mass of MCO₃ 

• • M_r =
  • M_r =   = 100.9 g mol^-1 

Step 4: Calculate the atomic mass of M in MCO₃ and deduction of the Group 2 metal

• • M_r = Σ(atomic masses)
  • 100.9 = M + 12.0 + (3 x 16.0)
  • M = 100.9 - 60.0 = 40.9 g mol^-1 
  • The closest Group 2 atomic mass is calcium at 40.1 g mol^-1, therefore the metal M is calcium

Hazards, risks and precautions

• The hazards associated with acids depend on the type and concentration of the acid
• Most dilute acids either require no hazard symbol or they are an irritant, so require the symbol to show they are harmful to health
  • Eye protection should be worn when handling
• Moderately concentrated acids are often corrosive
  • In addition to eye protection, gloves should also be worn
• Some concentrated acids, e.g. nitric acid, are oxidising which can cause or intensify a fire in contact with combustible materials
  • Eye protection and gloves are necessary when handling concentrated acids and the use of a fume cupboard is often required