How much graphite carbon must be burned in oxygen gas to produce 2.2 grams of carbon dioxide gas
To determine the amount of graphite carbon that must be burned in oxygen gas to produce 2.2 grams of carbon dioxide gas, we need to use stoichiometry and balanced chemical equations.
1. Start by writing the balanced chemical equation for the combustion of graphite carbon (C) in oxygen gas (O2) to form carbon dioxide gas (CO2):
C + O2 -> CO2
2. Determine the molar mass of carbon dioxide by adding up the atomic masses of carbon (C) and oxygen (O):
Molar mass of CO2 = (1 mol C) + (2 mol O) = 12.01 g/mol + 2 * 16.00 g/mol = 44.01 g/mol
3. Use stoichiometry to calculate the amount of carbon dioxide produced when 1 mol of carbon is burned:
1 mol C -> 1 mol CO2
4. Calculate the amount of carbon dioxide produced when 12.01 g (the molar mass of carbon) is burned:
12.01 g C * (1 mol CO2 / 1 mol C) * (44.01 g CO2 / 1 mol CO2) = 528.33 g CO2
5. Now, we can determine the amount of graphite carbon required to produce 2.2 g of carbon dioxide:
2.2 g CO2 * (1 mol C / 44.01 g CO2) * (12.01 g C / 1 mol C) = 0.0597 g C
Therefore, approximately 0.0597 grams of graphite carbon must be burned in oxygen gas to produce 2.2 grams of carbon dioxide gas.