The given question is incomplete. The complete question is:
The combustion of propane (C3H8) in the presence of excess oxygen yields [tex]CO_2[/tex] and [tex]H_2O[/tex]
[tex]C_3H_8(g)+5O_2 (g)\rightarrow 3CO_2(g)+4H_2O (g)[/tex]
When only 2.5 mol of [tex]O_2[/tex] are consumed in order to complete the reaction, ________ mol of [tex]CO_2[/tex] are produced.
Answer: Thus when 2.5 mol of [tex]O_2[/tex] are consumed in their reaction, 1.5 mol of [tex]CO_2[/tex] are produced
Explanation:
The balanced chemical equation is:
[tex]C_3H_8(g)+5O_2 (g)\rightarrow 3CO_2(g)+4H_2O (g)[/tex]
According to stoichiometry :
5 moles of [tex]O_2[/tex] produce = 3 moles of [tex]CO_2[/tex]
Thus 2.5 moles of [tex]O_2[/tex] will produce = [tex]\frac{3}{5}\times 2.5=1.5[/tex] moles of [tex]CO_2[/tex]
Thus when 2.5 mol of [tex]O_2[/tex] are consumed in their reaction, 1.5 mol of [tex]CO_2[/tex] are produced
