Step 1: From the problem, the given combustion reaction is:
C8H18 + O2 → CO2 + H2O
This equation is not yet balanced. To balance it, we have to make sure that the number of elements on both sides is equal.
Balance C: We have 8 C on the reactant side and 1 C on the product side – add a coefficient of 8 to CO2:
C8H18 + O2 → 8 CO2 + H2O
Balance H: We have 18 H on the reactant side and 2 H on the product side – add a coefficient of 9 to H2O:
C8H18 + O2 → 8 CO2 + 9 H2O
Balance O: We have 2 O on the reactant side and 8(2) + 9 = 25 O on the product side – multiply the entire equation by 2 and add a coefficient of 25 to O2:
2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
Now that we have a balanced equation, we can proceed with the problem.
Determine the balanced chemical equation for this reaction. C8H18(g)+O2(g)→CO2(g)+H2O(g)
Enter the coefficients for each compound in order, separated by commas. For example, 1,2,3,4 would indicate one mole of C8H18, two moles of O2, three moles of CO2, and four moles of H2O.
0.280 mol of octane is allowed to react with 0.630 mol of oxygen. Which is the limiting reactant?
How many moles of water are produced in this reaction?
After the reaction, how much octane is left?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Limiting Reagent concept. If you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Wang's class at MISSOURI STATE.