Question

Using the following equation for the combustion of octane, calculate the heat associated with the combustion of 150.0 g of octane assuming complete combustion. The molar mass of octane is 114.33 g/mole. 2 C8H18 + 25 O2 ? 16 CO2 + 18 H2O ?H°rxn = -11018 kJ -578.2 kJ -903.4 kJ -803.1 kJ -11018 kJ -7228 kJ

          Using the following equation for the combustion of octane, calculate the heat associated with the combustion of 150.0 g of octane assuming complete combustion. The molar mass of octane is 114.33 g/mole.

2 C8H18 + 25 O2 ? 16 CO2 + 18 H2O
?H°rxn = -11018 kJ

-578.2 kJ
-903.4 kJ
-803.1 kJ
-11018 kJ
-7228 kJ

Show more…

Using the following equation for the combustion of octane, calculate the heat associated with the combustion of 150.0 g of octane assuming complete combustion. The molar mass of octane is 114.33 g/mole.

2 C8H18 + 25 O2 ? 16 CO2 + 18 H2O
?H°rxn = -11018 kJ

-578.2 kJ
-903.4 kJ
-803.1 kJ
-11018 kJ
-7228 kJ

Added by Rebecca D.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Amita Prajapat

03/26/2022

Step 1

0 g. We can do this by dividing the mass of octane by its molar mass: 150.0 g / 114.33 g/mol = 1.31 mol The heat of reaction (ΔHrxn) given is for the combustion of 2 moles of octane. So, the heat of combustion for 1 mole of octane would be half of this: -11018 Show more…

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Using the following equation for the combustion of octane, calculate the heat associated with the combustion of 150.0 g of octane assuming complete combustion. The molar mass of octane is 114.33 g/mole. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ -578.2 kJ -903.4 kJ -803.1 kJ -11018 kJ -7228 kJ

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