For the reaction
? C6H6 + ? O2 ↽⇀? CO2 + ? H2O
a maximum of ? moles of CO2 could be
formed from 6.38 mol of C6H6 and 6.03 mol
of O2.
Answer in units of mol
B==-D {0} mol
5665
To determine the maximum number of moles of CO2 that can be formed from a given amount of C6H6 (benzene) and O2 (oxygen), we need to look at the balanced chemical equation for the reaction. The coefficients in the balanced equation can help us calculate the moles of each substance involved.
The balanced equation for the combustion of benzene is:
1 C6H6 + 15 O2 → 6 CO2 + 3 H2O
According to the balanced equation, for every 1 mole of benzene (C6H6), we need 15 moles of oxygen (O2) to produce 6 moles of carbon dioxide (CO2) and 3 moles of water (H2O).
Now, let's calculate the moles of CO2 that can be formed based on the given amounts of C6H6 and O2:
Given:
Moles of C6H6 = 6.38 mol
Moles of O2 = 6.03 mol
First, we need to determine the limiting reactant, which is the reactant that is completely consumed and determines the maximum amount of product formed. To do this, we compare the moles of C6H6 and O2 using their coefficients in the balanced equation.
Moles of CO2 formed from C6H6 = (6.38 mol C6H6) × (6 mol CO2 / 1 mol C6H6) = 38.28 mol CO2
Moles of CO2 formed from O2 = (6.03 mol O2) × (6 mol CO2 / 15 mol O2) ≈ 2.41 mol CO2
Since we have a lesser number of moles of CO2 formed from O2 (2.41 mol), it indicates that O2 is the limiting reactant. Therefore, 2.41 moles of CO2 can be formed from 6.38 moles of C6H6 and 6.03 moles of O2.
Therefore, the maximum number of moles of CO2 that can be formed is 2.41 mol.