The burning of gasoline in automobile engines is a chemical reaction. In light of the law of conservation of mass, explain what happens to the gasoline in your car's tank as you drive.

answer

watching

170

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Christian TusoLv10

27 Nov 2020

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

4. About 30% of crude oil is processed eventually into automobile gasoline. As petroleum prices rise and resources dwindle, alternatives must be found. However, automobile engines can be tuned so that they will run on simple alcohols. Methanol and ethanol can be derived from coal or plant biomass, respectively. While the alcohols produce fewer pollutants than gasoline, they also reduce the travel radius of a tank of fuel. What percent increase in the size of the fuel tank is needed to give an equivalent travel radius if gasoline is replaced by alcohol? Base your calculations on 40 kJ/g of gasoline having a specific gravity of 0.84, and the product water as a gas. Make the calculations for a) Methanol b) ethanol â

2 questions pleaseeee helppp

In Europe, gasoline efficiency is measured in km/L. If your car's gas mileage is 27.0mi/gal , how many liters of gasoline would you need to buy to complete a 142-km trip in Europe? Use the following conversions: 1km=0.6214mi and 1gal=3.78L.

While in Europe, if you drive 101km per day, how much money would you spend on gas in one week if gas costs 1.10 euros per liter and your car's gas mileage is 37.0mi/gal ? Assume that 1euro=1.26dollars.