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?

1.94 g

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-molStandard temperature: T = 273.15 KStandar pressure: 0.986923 atmn = 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 molesmolar mass of CO₂ = 44.01 g/molmass = 0.0440 mol × 44.01 g/mol = 1.94 g ← answer

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