Assume that a car burns octane, C8 H18(d=0.703 g / cm^3). (a) Write the balanced equation for b

Assume that a car burns octane, C8 H18(d=0.703 g / cm^3)....

Assume that a car burns octane, $\mathrm{C}_{8} \mathrm{H}_{18}\left(d=0.703 \mathrm{~g} / \mathrm{cm}^{3}\right)$. (a) Write the balanced equation for burning octane in air. forming $\mathrm{CO}_{2}$ and $\mathrm{H}_{2} \mathrm{O} .$ (b) The car has a fuel efficiency of 32 miles per gallon of octane; determine the volume of $\mathrm{CO}_{2}$ at $25{ }^{\circ} \mathrm{C}$ and $1.0 \mathrm{~atm}$ that is generated when the car goes on a 10 -mile trip.

Assume that a car burns octane, $\mathrm{C}_{8} \mathrm{H}_{18}\left(d=0.703 \mathrm{~g} / \mathrm{cm}^{3}\right)$.
(a) Write the balanced equation for burning octane in air. forming $\mathrm{CO}_{2}$ and $\mathrm{H}_{2} \mathrm{O} .$
(b) The car has a fuel efficiency of 32 miles per gallon of octane; determine the volume of $\mathrm{CO}_{2}$ at $25{ }^{\circ} \mathrm{C}$ and $1.0 \mathrm{~atm}$ that is generated when the car goes on a 10 -mile trip.

Key Concepts

Chemical Stoichiometry

Chemical stoichiometry involves calculating the quantitative relationships between reactants and products in a chemical reaction. It is used to determine the amounts in moles or mass of products released based on the known amounts of reactants consumed, establishing precise ratios required by the balanced chemical equation.

Combustion Reactions

A combustion reaction is a type of exothermic reaction in which a fuel, typically a hydrocarbon like octane, reacts with an oxidizer, usually oxygen, to produce carbon dioxide and water. Understanding combustion is critical for energy production, engine efficiency, and environmental impact assessments.

Balancing Chemical Equations

Balancing chemical equations is the process of ensuring that the number of atoms for each element is conserved before and after a reaction. This ensures compliance with the law of conservation of mass, which is essential for accurate stoichiometric calculations in chemical reactions.

Ideal Gas Law

The ideal gas law (PV = nRT) relates the pressure, volume, temperature, and number of moles of a gas. It is an essential tool for determining the volume of gases produced or consumed in chemical reactions under specified conditions, making it particularly useful in problems involving gas evolution.

Fuel Efficiency and Unit Conversions

Fuel efficiency expresses how effectively a vehicle converts a given volume of fuel into distance traveled. It often requires unit conversions, such as converting fuel volume to mass using density or miles to appropriate distance units, to relate the amount of fuel consumed to the amount of products generated in combustion reactions.

Transcript

00:01 Let us discuss the first part of the problem, which is combustion of octane.

00:07 Combession of octane forms carbon dioxide and the water.

00:11 The equation is c8h18 plus o2 gives rise to co2 plus h2o.

00:38 As there are 8 carbon atoms multiply with 8 near the carbon dioxide, as there are 18 hydrogen atoms multiply with 9 near the h2o.

00:49 Totally, there are 25 oxygen atoms on the right side.

00:53 It will be 25 by 2.

00:59 This is the balanced equation.

01:03 Coming to the second part of the problem, we have to calculate the volume of carbon dioxide from the given data.

01:14 The given data is fuel efficiency of the car is equal to 32 miles per gallon.

01:43 The temperature is given as 25 degrees celsius which can be converted into kelvin.

01:48 25 plus 273 .15 equals to 298 .15 kelvin.

02:08 Pressure is given as a 1 .5.

02:10 One atmosphere.

02:13 Density of octane is 0 .703 gram per cc.

02:28 We have to convert the volume of octane in terms of gallons.

02:33 So 32 miles per one gallon.

02:57 The volume of octane required for car to travel 10 miles is equal to 10 into 1 by 32.

03:50 The value equals to 0 .33 galones...

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