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Calculate the mole and mass in kg of CO2 formed by the combustion of 20.00kg carbon in excess o2 (c=12.00 and O=16.00)
Accepted Answer
1. Balanced Chemical Equation:
The combustion of carbon in excess oxygen produces carbon dioxide:
C + O₂ → CO₂
2. Moles of Carbon:
Molar mass of carbon (C) = 12.00 g/mol
Moles of carbon = (mass of carbon) / (molar mass of carbon) = (20.00 kg
1000 g/kg) / (12.00 g/mol) = 1666.67 mol
3. Moles of Carbon Dioxide:
From the balanced equation, 1 mole of carbon produces 1 mole of carbon dioxide.
Therefore, 1666.67 mol of carbon produces 1666.67 mol of carbon dioxide.
4. Mass of Carbon Dioxide:
Molar mass of carbon dioxide (CO₂) = 12.00 g/mol + (2
16.00 g/mol) = 44.00 g/mol
Mass of carbon dioxide = (moles of CO₂)
(molar mass of CO₂) = (1666.67 mol)
(44.00 g/mol) = 73333.33 g = 73.33 kg
Answer:
Moles of CO₂ formed = 1666.67 mol
Mass of CO₂ formed = 73.33 kg
The combustion of carbon in excess oxygen produces carbon dioxide:
C + O₂ → CO₂
2. Moles of Carbon:
Molar mass of carbon (C) = 12.00 g/mol
Moles of carbon = (mass of carbon) / (molar mass of carbon) = (20.00 kg
1000 g/kg) / (12.00 g/mol) = 1666.67 mol
3. Moles of Carbon Dioxide:
From the balanced equation, 1 mole of carbon produces 1 mole of carbon dioxide.
Therefore, 1666.67 mol of carbon produces 1666.67 mol of carbon dioxide.
4. Mass of Carbon Dioxide:
Molar mass of carbon dioxide (CO₂) = 12.00 g/mol + (2
16.00 g/mol) = 44.00 g/mol
Mass of carbon dioxide = (moles of CO₂)
(molar mass of CO₂) = (1666.67 mol)
(44.00 g/mol) = 73333.33 g = 73.33 kg
Answer:
Moles of CO₂ formed = 1666.67 mol
Mass of CO₂ formed = 73.33 kg
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