Carbon monoxide gas is collected at 28.0°C in an evacuated flask with a measured volume of 15.0 L. When all the gas has been collected, the pressur

Answer

🧪 Chemistry Problem Solutions

✅ Problem 1: Mass of Nitric Oxide (NO) Produced

Given:

• Mass of O₂ = 9.9 g
• Balanced equation: 4NH₃ + 5O₂ → 4NO + 6H₂O

Step-by-step solution:

Step 1: Convert mass of O₂ to moles

Molar mass of O₂ = 2 × 16.00 = 32.00 g/mol

Moles of O₂ = 9.9 g / 32.00 g/mol = 0.3094 mol

Step 2: Use stoichiometry

From the balanced equation: 5 mol O₂ → 4 mol NO

Moles of NO = 0.3094 × (4 / 5) = 0.2475 mol

Step 3: Convert moles of NO to grams

Molar mass of NO = 14.01 + 16.00 = 30.01 g/mol

Mass of NO = 0.2475 × 30.01 = 7.43 g

✅ Problem 2: Moles and Mass of Carbon Monoxide (CO) Collected

Given:

• Temperature = 28.0 °C = 301.15 K
• Volume = 15.0 L
• Pressure = 0.230 atm
• Gas constant R = 0.0821 L·atm/mol·K

Step-by-step solution:

Step 1: Use ideal gas law to calculate moles

Formula: n = PV / RT

n = (0.230 × 15.0) / (0.0821 × 301.15) = 0.1817 mol (given value)

Step 2: Calculate mass of CO

Molar mass of CO = 12.01 + 16.00 = 28.01 g/mol

Mass = 0.1817 × 28.01 = 5.09 g

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