One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH 3 to NO: 4 NH 3 (g) + 5 O 2 (g) → 4 NO(g) + 6 H 2 O(g) In a certain experiment, 2.00 g of NH 3 reacts with 2.50 g of O 2 . (d) Show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass.

Hey everyone in this example, we're told that ammonia can be converted to nitric acid in the given reaction below. And one step in that process is the conversion of ammonia to nitrogen monoxide. We're told that this reaction was studied by reacting 4.50 g of ammonia with 3.20 g of oxygen gas. And after the react and reached reached completion, we have 2.40 g of nitrogen monoxide and 2.16 g of oxygen gas that was produced and 3.14 g of ammonia. That has remained. We need to show how this is consistent with the law of conservation of mass. So we should recall for our law of conservation of mass that we have. The two main principles wherein the first principle are mass of our components in our reaction should be conserved, not changed. And for the second important principle of our law here we have that the mass of our reactant should equal the mass of our products. So according to the prompt, our reactant where we have 4.50 g of ammonia and 3.20 g of oxygen, which are our initial masses before our reaction begins. These equal a sum of 7.70 g. So this is our mass Before the reaction occurs. And now we want to find our mass after the reaction. And so what we're going to do is take our mass of nitrogen monoxide given in the prompt as 2.40 g and add that to our mass of oxygen gas Given in the prompt as 2.16g, Which we will also add to the amount of Ammonia that has remained after our reaction went through. And so in the prompt that that that is given as 3.14 g of ammonia. And so this equals a value also of 7. g, which is our mass after our reaction. And so we can say that therefore our mass of our reactant is equal to our mass of our products plus access reactant, which is our ammonia. Thus the mass of components of the reaction is conserved. And so this will be our final answer to complete this example to show how a reaction here is consistent with the law of conservation of mass. So if you have any questions, please leave them down below. Otherwise, I will see everyone in the next practice video.

Ch.3 - Chemical Reactions and Reaction Stoichiometry

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Brown 14th Edition

Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 80d

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Chapter 3, Problem 80d

One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH₃ to NO: 4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g) In a certain experiment, 2.00 g of NH₃ reacts with 2.50 g of O₂. (d) Show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass.

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Calculate the molar mass of NH3 (ammonia) and O2 (oxygen) to convert the given masses from grams to moles. The molar mass of NH3 is approximately 17.03 g/mol and for O2 it is approximately 32.00 g/mol.

Using the stoichiometry of the balanced chemical equation, determine the theoretical amount of O2 required to completely react with the given amount of NH3. Use the mole ratio from the balanced equation, which is 5 moles of O2 for every 4 moles of NH3.

Compare the actual amount of O2 provided (2.50 g converted to moles) to the theoretical amount needed. Determine which reactant is the limiting reactant, which is the reactant that will be completely consumed and thus limits the extent of the reaction.

Calculate the total mass of the products formed by the reaction using the stoichiometry of the balanced equation and the amount of the limiting reactant. Convert moles of products back to grams using their respective molar masses.

Verify the law of conservation of mass by comparing the total mass of the reactants to the total mass of the products. The sum of the masses of the reactants should equal the sum of the masses of the products.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Law of Conservation of Mass

The Law of Conservation of Mass states that mass is neither created nor destroyed in a chemical reaction. This principle implies that the total mass of the reactants must equal the total mass of the products. In the context of the given reaction, verifying this law involves ensuring that the sum of the masses of ammonia and oxygen before the reaction equals the sum of the masses of nitrogen monoxide and water produced.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on balanced chemical equations. It allows chemists to determine the proportions of substances involved in a reaction. In this case, stoichiometry will help in calculating the theoretical yield of products from the given amounts of ammonia and oxygen, which is essential for demonstrating the conservation of mass.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between the mass of a substance and the number of moles, which is necessary for stoichiometric calculations. In this problem, calculating the molar masses of NH3 and O2 will enable the determination of how many moles are reacting, facilitating the verification of the conservation of mass.

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Molar Mass Concept

Related Practice

The fizz produced when an Alka-Seltzer tablet is dissolved in water is due to the reaction between sodium bicarbonate 1NaHCO32 and citric acid 1H3C6H5O72: 3 NaHCO31aq2 + H3C6H5O71aq2¡ 3 CO21g2 + 3H2O1l2 + Na3C6H5O71aq2 In a certain experiment 1.00 g of sodium bicarbonate and 1.00 g of citric acid are allowed to react. (a) Which is the limiting reactant? (b) How many grams of carbon dioxide form? (c) How many grams of the excess reactant remain after the limiting reactant is completely consumed?

One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4 NH31g2 + 5 O21g2¡4 NO1g2 + 6 H2O1g2 In a certain experiment, 2.00 g of NH3 reacts with 2.50 g of O2. (a) Which is the limiting reactant?

Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 3.50 g of sodium carbonate is mixed with one containing 5.00 g of silver nitrate. How many grams of sodium carbonate are present after the reaction is complete? How many grams of sodium nitrate are present after the reaction is complete?

Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 3.50 g of sodium carbonate is mixed with one containing 5.00 g of silver nitrate. How many grams of silver carbonate are present after the reaction is complete?

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Textbook Question

Solutions of sulfuric acid and lead(II) acetate react to form solid lead(II) sulfate and a solution of acetic acid. If 5.00 g of sulfuric acid and 5.00 g of lead(II) acetate are mixed, calculate the number of grams of sulfuric acid and grams of acetic acid present in the mixture after the reaction is complete.

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