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Ch.3 - Chemical Reactions and Reaction Stoichiometry

Chapter 3, Problem 114b

The source of oxygen that drives the internal combustion engine in an automobile is air. Air is a mixture of gases, principally N2179%2 and O2120%2. In the cylinder of an automobile engine, nitrogen can react with oxygen to produce nitric oxide gas, NO. As NO is emitted from the tailpipe of the car, it can react with more oxygen to produce nitrogen dioxide gas. (b) Both nitric oxide and nitrogen dioxide are pollutants that can lead to acid rain and global warming; collectively, they are called 'NOx' gases. In 2009, the United States emitted an estimated 19 million tons of nitrogen dioxide into the atmosphere. How many grams of nitrogen dioxide is this?

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Hello in this video, we're going to be doing some dimensional analysis. So in this problem, we can see that we're talking about aspirin and we're going to be given some values in some type of unit and we want to be converted into some type of other unit. So first I want you guys to notice that were given the 40, tons her year and we want to convert this mass two ounces. So we only want to focus on our mass, which is going to be our tons. So was a direct conversion from tons, two ounces. I'm not sure if you guys know but I have no clue. So what I'm gonna do is not a direct conversion, we're going to take it in baby steps. So first I'll go from tons, two kg, £2 and then two oz. These are just conversions that I know you can do maybe in two steps or one step or even more steps in this. But these are just conversions that I kind of know already. So that's why I'll be using this method or this road map here. So for my dimensional analysis, I'm going to first start off with meg Given Which is going to be my 1000 tons. So we're starting here, then I'm going to go to kilograms. So for every one ton I'm going to have 1000 kg. So you can see that the tense is going to go ahead and catch up perfectly. So It's all being multiplied. Alright, so done with the kg. Now we're gonna go £2. So For every one kg there's going to be £2.20. And again, sorry, this is A B. All right, so you can see how our kilogram unit will cancel out nicely. So we're done with the pound. Lastly our last stop will be our ounces Again. This is being multiplied. Alright, so every £1 There's going to be ounces. So answers abbreviated is cozy and you can see here again that the pounds will cancel it nicely and the answer will have the ounces as our units and that's exactly what the problem asked for us is convert the mass two ounces. Alright, so putting this into my calculator, I'm going to go and get a value Of 1. Times 10 to the nine power ounces. And that is going to be my final answer for this problem.
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Textbook Question
A 3.50 g of an alloy which contains only lead and tin is dissolved in hot HNO3. Excess sulfuric acid is added to this solution and 1.57g of PbSO4(s) is obtained. (b) Assuming all the lead in the alloy reacted to form PbSO4, what was the amount, in grams, of lead and tin in the alloy respectively?
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Textbook Question

Hydrogen cyanide, HCN, is a poisonous gas. The lethal dose is approximately 300 mg HCN per kilogram of air when inhaled. (a) Calculate the amount of HCN that gives the lethal dose in a small laboratory room measuring 3.5 * 4.5 * 2.5 m. The density of air at 26 C is 0.00118 g>cm3.

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Textbook Question

Hydrogen cyanide, HCN, is a poisonous gas. The lethal dose is approximately 300 mg HCN per kilogram of air when inhaled. (c) HCN forms when synthetic fibers containing Orlon® or Acrilan ® burn. Acrilan® has an empirical formula of CH2CHCN, so HCN is 50.9% of the formula by mass. A rug measures 3.5 * 4.5 m and contains 850 g of Acrilan® fibers per square yard of carpet. If the rug burns, will a lethal dose of HCN be generated in the room? Assume that the yield of HCN from the fibers is 20% and that the carpet is 50% consumed.

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Textbook Question

The source of oxygen that drives the internal combustion engine in an automobile is air. Air is a mixture of gases, principally N2(79%) and O2(20%). In the cylinder of an automobile engine, nitrogen can react with oxygen to produce nitric oxide gas, NO. As NO is emitted from the tailpipe of the car, it can react with more oxygen to produce nitrogen dioxide gas. (c) The production of NOx gases is an unwanted side reaction of the main engine combustion process that turns octane, C8H18, into CO2 and water. If 85% of the oxygen in an engine is used to combust octane and the remainder used to produce nitrogen dioxide, calculate how many grams of nitrogen dioxide would be produced during the combustion of 500 g of octane.

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Textbook Question

The thermite reaction, Fe2O3 + Al → Al2O3 + Fe produces so much heat that the Fe product melts. This reaction is used industrially to weld metal parts under water, where a torch cannot be employed. It is also a favorite chemical demonstration in the lecture hall (on a small scale). (b) Calculate how many grams of aluminum are needed to completely react with 500.0 g of Fe2O3 in this reaction.

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Textbook Question

The thermite reaction, Fe2O3 + Al S Al2O3 + Fe produces so much heat that the Fe product melts. This reaction is used industrially to weld metal parts under water, where a torch cannot be employed. It is also a favorite chemical demonstration in the lecture hall (on a small scale). (d) If you performed the reverse reaction— aluminum oxide plus iron makes iron oxide plus aluminum—would that reaction have heat as a reactant or a product?

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