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Nitrous oxide $\left(\mathrm{N}_{2} \mathrm{O}\right)$ is also called "laughing gas." It can be prepared by the thermal decomposition of ammonium nitrate $\left(\mathrm{NH}_{4} \mathrm{NO}_{3}\right) .$ The other product is $\mathrm{H}_{2} \mathrm{O} .$ (a) Write a balanced equation for this reaction.(b) How many grams of $\mathrm{N}_{2} \mathrm{O}$ are formed if 0.46 mole of $\mathrm{NH}_{4} \mathrm{NO}_{3}$ is used in the reaction?

a) $\mathrm{NH}_{4} \mathrm{NO}_{3} \rightarrow \mathrm{N}_{2} \mathrm{O}+2 \mathrm{H}_{2} \mathrm{O}$b) $20.25 \mathrm{g}$

Chemistry 101

Chapter 3

Mass Relationships in Chemical Reactions

Chemical reactions and Stoichiometry

Carleton College

University of Central Florida

University of Maryland - University College

Brown University

Lectures

04:02

A chemical reaction is a process that leads to the transformation of one set of chemical substances to another. Chemical reactions can be either spontaneous, requiring no input of energy, or non-spontaneous, typically following the input of some type of energy, such as heat, light or electricity. Chemical reactions are usually characterized by a chemical change, and they yield one or more products after the reaction is complete. Chemical reactions are described with chemical equations, which symbolically present the starting materials, end products, and sometimes intermediate products and reaction conditions. Chemical reactions happen at a characteristic reaction rate at a given temperature and chemical concentration. Typically, reaction rates increase with increasing temperature because there is more thermal energy available to reach the activation energy necessary for breaking bonds between atoms.

08:02

In chemistry, a combination reaction is a chemical reaction in which two or more reactants combine to form more than one product. In a decomposition reaction, one reactant splits into two or more products.

04:12

Nitrous oxide $\left(\math…

01:16

Laughing gas (dinitrogen m…

04:30

01:02

Nitrous oxide, $\mathrm{N…

05:10

Dinotrogen monoxide, commo…

So for this problem, we have the decomposition of ammonium nitrate and we're supposed to have two parts in the first part. You want to balance the equation for the decomposition of ammonium nitrate, so we know that he only reacted in this case. It's going to be running my treat. And we know that the product has given to us in the problem or nitrous oxide as well as each. You know that we have the products in the reactors. We need to balance the equation now. So first we look to the nitrogen. Nitrogen is balanced. We have two on each side. Then we look to the hydrogen. We have four on the left hand side and only two on the right. So to make it even put it to in front of the H 20 And now we have for each side. Now, lastly, be verify oxygen. So in the left hand side, we have three oxygen on the bright and saidi of one plus to because of this new coefficient, to know if three on both sides and the entire equation is balanced. So this he's the final balanced. That is the answer to part a never part B. We have to do some soy geometry and some dimensional analysis because we have 0.46 moles of NH four and 03 being formed, and we want to find any each of 0.46 molds of NH 403 being used and you want to find how many grams event to reform. So the first thing that we need to do is we need to find the more massive nitrous oxide that we can then use that in order to solve this problem. So we have to nitrogen just 14 point no. One grams from all minute oxygen, which is 16 point hello. And so then when you calculate this out, we'll get that the molar mass is 44 0.2 grams. So now that we have the molar mass of n 20 we can then do the dimensional analysis. So we know that we're starting with 0.46 moles, ammonium nitrate and then, as we can see from the balanced equation, the multiple ratio between n 20 and ammonium nitrate is 1 to 1, because both of those coefficients are one. And then the last thing we need to do is multiplied by the molar mass, so we get grams of into row in serving bowls. If you multiply the more mass, which is 44 point. Oh, to like we calculated we get 20.0. Grams per into that, it's the final answer.

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