The combustion of ethane (C2H6) produces carbon dioxide and steam:
2C2H6+702 yields 4CO2 +6H2O
How many moles of CO2 are produced when 5.30 mol of ethane are burned in an excess of oxygen?
mols C2H6 = 5.30
Using the coefficients in the balanced equation, convert mols C2H6 to mols CO2.
5.30 x (4 mol CO2/2 mol C2H6) = 5.30 x (4/2) = ?
10.6
10.6 moles of CO2 are produced when 5.30 mol of ethane are burned in an excess of oxygen.
To find the number of moles of CO2 produced when 5.30 mol of ethane are burned, we need to use the balanced chemical equation and apply stoichiometry.
The balanced equation is:
2C2H6 + 7O2 -> 4CO2 + 6H2O
From the equation, we can see that 2 moles of ethane (C2H6) produce 4 moles of CO2. This means the ratio is 2:4, or simplified 1:2.
So, for every 1 mole of ethane, 2 moles of CO2 are produced.
Since we have 5.30 moles of ethane, we can multiply this value by the ratio to find the number of moles of CO2 produced:
5.30 mol C2H6 * (2 mol CO2 / 1 mol C2H6) = 10.60 mol CO2
Therefore, when 5.30 mol of ethane are burned, 10.60 mol of CO2 are produced.