Question

Carbon monoxide (CO) gas reacts with oxygen

(O2) gas to produce carbon dioxide (CO2) gas. If
1.00 L of carbon monoxide reacts with excess
oxygen at standard temperature and pressure,
what volume of carbon dioxide is produced?
What mass of carbon dioxide is produced?

Answer 1

1.00L

1.96G

0.500mol

0.750mol

16.8L

Step-by-step explanation:

Answer 2

• 1.94 g

Step-by-step explanation:

1) Chemical equation (unbalanced)

• CO (g) + O₂ (g) → CO₂ (g)

2) Balanced chemical equation:

• 2CO (g) + O₂ (g) → 2CO₂ (g)

3) Mole ratio:

• 2 mol CO : 2 mol CO₂, which is the same as 1 : 1.

4) Volume ratio:

Since the reaction is carried out at constant pressure and temperature, the volume ratios are equal to the mole ratios. Then:

• 1 liter CO : 1 liter CO₂

Hence, 1.00 liter of CO gas produces 1.00 liter of CO₂

3) Mass of carbon dioxide:

a) Use ideal gas equation to convert 1.00 liter CO₂ produced to moles:

• pV = nRT ⇒ n = pV / (RT)

• R = 0.08206 atm-liter/k-mol

• Standard temperature: T = 273.15 K

• Standar pressure: 0.986923 atm

• n = 0.986923 atm × 1.00 liter / (0.08206 atm-liter/K-mol × 273.15 K)

• n = 0.0440 mol

b) Convert moles to mass in grams

• mass in grams = molar mass × number of moles

• molar mass of CO₂ = 44.01 g/mol

• mass = 0.0440 mol × 44.01 g/mol = 1.94 g ← answer