We’re being asked to calculate the mass of octane (C8H18) consumed by the reaction of 8.5 g O2.
For this problem, we need to do the following steps:
Step 1: Write and balance a chemical equation for the given reaction.
Step 2: Calculate the mass of C8H18 consumed.
Step 1: From the problem, the given 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.
A major component of gasoline is octane (C8H18). When octane is burned in air, it chemically reacts with oxygen gas (O2) to produce carbon dioxide (CO2) and water (H2O).
What mass (grams) of octane is consumed by the reaction of 8.5 g of oxygen gas?
Round your answer to 2 significant digits.
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 Stoichiometry concept. You can view video lessons to learn Stoichiometry. Or if you need more Stoichiometry practice, you can also practice Stoichiometry practice problems.
What is the difficulty of this problem?
Our tutors rated the difficulty ofA major component of gasoline is octane (C8H18). When octane...as medium difficulty.
How long does this problem take to solve?
Our expert Chemistry tutor, Dasha took 5 minutes and 46 seconds to solve this problem. You can follow their steps in the video explanation above.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Saber's class at TAMU.