Question

C3H8 + O2 → CO2 + H2O

In the UNBALANCED chemical reaction for the combustion of propane, if 5.3 moles of carbon dioxide is produced, how many moles of oxygen reacted?

options:
A) 8.83 moles
B) 5.9 moles
C) 2.7 moles
D) 7 moles

Answer 1

To find the number of moles of oxygen that reacted with propane to produce 5.3 moles of CO2, we use the balanced combustion equation. It shows a 3:5 ratio of CO2 to O2, leading to the calculation that 8.83 moles of O2 reacted.

To determine the number of moles of oxygen that reacted to produce 5.3 moles of carbon dioxide in the combustion of propane, we must first write and balance the chemical equation:

C3H8 + 5O2 → 3CO2 + 4H2O
From the balanced equation, the stoichiometric ratio between CO2 and O2 is 3:5. Therefore, for every 3 moles of CO2 produced, 5 moles of O2 are consumed. Using simple proportions we find:

1. For 3 moles of CO2, 5 moles of O2 are used.
2. For 5.3 moles of CO2, X moles of O2 are used.

By cross-multiplying and solving for X, we get:

X = (5 moles of O2 / 3 moles of CO2) × 5.3 moles of CO2 = 8.83 moles of O2

Thus, the correct answer is option A) 8.83 moles.

Answer 2

Step-by-step explanation:

Balance the following equation: C3H8 + O2 ----> CO2 + H2O. (There will be no need for state symbols.) First of all, to balance these equations, list the number of each atom, for both sides of the equation. In this example, it would be: The first step would be to balance out the carbons on the products side by multiplying CO2 by 3. The balanced chemical equation for C3H8 +O2 = CO2 + H2O is C3H8 +5O2 = 3CO2 +4H2O. This is the chemical reaction in which C3H8 or propane burns in air or oxygen to produce carbon dioxide and water.