# Part A Determine the balanced chemical equation for this reaction. C8H18(g)+O2(g)...

## Question:

Part A

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.

2,25,16,18

Correct It is important to balance a chemical equation before using it for calculations. Checking that equations are balanced will help you avoid many errors in chemistry problems

. Balanced chemical equation

2C8H18(g)+25O2(g) ?,16CO2(g)+18H2O(g

Part B

0.240 mol of octane is allowed to react with 0.700 mol of oxygen. Which is the limiting reactant

octane

oxygen

Part Correct

Now that you have identified oxygen as the limiting reactant, you can use the number of moles of oxygen to find the numbers of moles of all the other substances.

Part C

How many moles of water are produced in this reaction?

H2O produced = 0.504 mol

All attempts used; correct answer displayed

Part D I need the anwser for part D

After the reaction, how much octane is left?

these all of my wrong answers

= 0.777mole

moles of C8H18 remaining = 0.1896 octane

moles of C8H18 remaining = 0.1896g

moles of C8H18 remaining = 0.196g

## Combustion of Hydrocarbons:

A combustion reaction involves the exothermic oxidation of a fuel by an oxidant to form gaseous oxidized products. For hydrocarbons (the fuel) undergoing complete combustion in excess oxygen (the oxidant) this forms water and carbon dioxide as products. This reaction is the basis of all internal combustion engines in automobiles.

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Question A)

The balanced reaction equation for the complete combustion of octane is:

{eq}2C_8H_{18} + 25O_2 \rightarrow 16CO_2 (g) + 18H_2O (g)...