Balance the following equations. (c) The burning of rocket fuel: C 2 H 8 N 2 + N 2 O 4 --> N 2 + CO 2 + H 2 O

Step 1: Identify the number of atoms of each element on both sides of the equation. In the reactants, we have 2 Carbon (C), 8 Hydrogen (H), 4 Nitrogen (N), and 4 Oxygen (O) atoms. In the products, we have 2 Nitrogen (N), 1 Carbon (C), 2 Oxygen (O), and 2 Hydrogen (H) atoms.. Step 2: Start balancing the equation by adjusting the coefficients of the compounds. Begin with the element that appears in the least number of compounds. In this case, start with Carbon (C). To balance the Carbon atoms, place a coefficient of 2 in front of CO 2 on the product side.. Step 3: Next, balance the Hydrogen atoms. To do this, place a coefficient of 4 in front of H 2 O on the product side.. Step 4: Now, balance the Nitrogen atoms. To do this, place a coefficient of 3 in front of N 2 on the product side.. Step 5: Finally, balance the Oxygen atoms. To do this, place a coefficient of 5 in front of N 2 O 4 on the reactant side. Now, the equation should be balanced with 2 Carbon (C), 8 Hydrogen (H), 10 Nitrogen (N), and 10 Oxygen (O) atoms on both sides of the equation.

Balance the following equations. (c) The burning of rocket fuel: C 2 H 8 N 2 + N 2 O 4 --> N 2 + CO 2 + H 2 O

Hey everyone. We're asked to balance the given chemical reaction first. Let's go ahead and count the number of atoms we have on both sides. Starting off with our react inside. We have one of nickel, one of hydrogen, one of nitrogen And three of oxygen. Looking at our product side, we have one of nickel as well, two of hydrogen, three of nitrogen and nine of oxygen only. Our nickel is balanced out. Let's first start off by balancing out our hydrogen. So if we add a coefficient of two prior to our nitric acid, we then are able to change our hydrogen into two, our nitrogen into two as well, And our oxygen's into six. Since we still need to change our nitrogen and oxygen's, this means we have to change The coefficient that we just inputted, which is R two. So instead of two, we can then go ahead and input a four prior to our nitric acid. And when we do that, we change our hydrogen into four, Our nitrogen into four as well. And our oxygen's into 12. Now that we've done this, we can adjust accordingly and look at our product side, we can add a coefficient of two prior to our water. And when we do this, we end up with four of hydrogen and our oxygen's changed from 9 to 10. Lastly, all we need to do is fix our nitrogen and our oxygen's and we can do that by fixing our nitrogen dioxide. So when we add a two prior to nitrogen dioxide, We end up with four of nitrogen And 12 of oxygen. So our balanced chemical reaction is going to be as such. So I hope this made sense and let us know if you have any questions.

Balance the following equations. (c) The burning of rocket fuel: C2H8N2 + N2O4 --> N2 + CO2 + H2O

Step 1: Identify the number of atoms of each element on both sides of the equation. In the reactants, we have 2 Carbon (C), 8 Hydrogen (H), 4 Nitrogen (N), and 4 Oxygen (O) atoms. In the products, we have 2 Nitrogen (N), 1 Carbon (C), 2 Oxygen (O), and 2 Hydrogen (H) atoms. Step 2: Start balancing the equation by adjusting the coefficients of the compounds. Begin with the element that appears in the least number of compounds. In this case, start with Carbon (C). To balance the Carbon atoms, place a coefficient of 2 in front of CO 2 on the product side. Step 3: Next, balance the Hydrogen atoms. To do this, place a coefficient of 4 in front of H 2 O on the product side. Step 4: Now, balance the Nitrogen atoms. To do this, place a coefficient of 3 in front of N 2 on the product side. Step 5: Finally, balance the Oxygen atoms. To do this, place a coefficient of 5 in front of N 2 O 4 on the reactant side. Now, the equation should be balanced with 2 Carbon (C), 8 Hydrogen (H), 10 Nitrogen (N), and 10 Oxygen (O) atoms on both sides of the equation.

Ch.3 - Mass Relationships in Chemical Reactions

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McMurry 8th Edition

Ch.3 - Mass Relationships in Chemical Reactions

Problem 39c

Chapter 3, Problem 39c

Balance the following equations. (c) The burning of rocket fuel: C₂H₈N₂ + N₂O₄ --> N₂ + CO₂ + H₂O

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Step 1: Identify the number of atoms of each element on both sides of the equation. In the reactants, we have 2 Carbon (C), 8 Hydrogen (H), 4 Nitrogen (N), and 4 Oxygen (O) atoms. In the products, we have 2 Nitrogen (N), 1 Carbon (C), 2 Oxygen (O), and 2 Hydrogen (H) atoms.

Step 2: Start balancing the equation by adjusting the coefficients of the compounds. Begin with the element that appears in the least number of compounds. In this case, start with Carbon (C). To balance the Carbon atoms, place a coefficient of 2 in front of CO₂ on the product side.

Step 3: Next, balance the Hydrogen atoms. To do this, place a coefficient of 4 in front of H₂O on the product side.

Step 4: Now, balance the Nitrogen atoms. To do this, place a coefficient of 3 in front of N₂ on the product side.

Step 5: Finally, balance the Oxygen atoms. To do this, place a coefficient of 5 in front of N₂O₄ on the reactant side. Now, the equation should be balanced with 2 Carbon (C), 8 Hydrogen (H), 10 Nitrogen (N), and 10 Oxygen (O) atoms on both sides of the equation.

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Key Concepts

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

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It involves using balanced chemical equations to determine the amounts of substances consumed and produced. Understanding stoichiometry is essential for balancing equations, as it ensures that the law of conservation of mass is upheld.

Balancing Chemical Equations

Balancing chemical equations involves adjusting the coefficients of reactants and products to ensure that the number of atoms of each element is the same on both sides of the equation. This process is crucial because it reflects the conservation of mass, indicating that matter is neither created nor destroyed in a chemical reaction. Techniques such as the inspection method or algebraic methods can be used to achieve balance.

Combustion Reactions

Combustion reactions are a type of chemical reaction where a substance (usually a hydrocarbon) reacts with oxygen to produce carbon dioxide and water, releasing energy in the form of heat and light. In the context of the given equation, understanding the nature of combustion is important for identifying the products formed and the stoichiometric relationships involved in the reaction.