Acetylene (C 2 H 2 ) and nitrogen (N 2 ) both contain a triple bond, but they differ greatly in their chemical properties. (c) Write balanced chemical equations for the complete oxidation of N 2 to form N 2 O 5 (g) and of acetylene to form CO 2 (g) and H 2 O(g). Write a balanced chemical equation for the complete oxidation of acetylene to form CO 2 (g) and H 2 O(g).

Hi everyone here we have a question asking us to write a balanced chemical equation for the complete oxidation of chlorine gas to form solid Dick Loreen tri oxide. So we have our korean gas plus oxygen forming solid die chlorine tri oxide. And if we look at our left, we see that our oxygen is in multiples of two. And on the right we have a three. So we need to make that an even number. So to do that, we're just going to put a two in front of it. And now we have six oxygen's on the right and we need six on the left. So we're going to put a three in front of our 02 and then we have four chlorine is on the right and two on the left. So we're going to put a two in front of our chlorine. And that is our final balanced equation. Thank you for watching. Bye.

Ch.8 - Basic Concepts of Chemical Bonding

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Brown 14th Edition

Ch.8 - Basic Concepts of Chemical Bonding

Problem 105c2

Chapter 8, Problem 105c2

Acetylene (C₂H₂) and nitrogen (N₂) both contain a triple bond, but they differ greatly in their chemical properties. (c) Write balanced chemical equations for the complete oxidation of N₂ to form N₂O₅(g) and of acetylene to form CO₂(g) and H₂O(g). Write a balanced chemical equation for the complete oxidation of acetylene to form CO₂(g) and H₂O(g).

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Identify the reactants and products for the oxidation reactions. For nitrogen, the reactant is \( N_2 \) and the product is \( N_2O_5 \). For acetylene, the reactant is \( C_2H_2 \) and the products are \( CO_2 \) and \( H_2O \).

Write the unbalanced chemical equations for each reaction. For nitrogen: \( N_2 + O_2 \rightarrow N_2O_5 \). For acetylene: \( C_2H_2 + O_2 \rightarrow CO_2 + H_2O \).

Balance the nitrogen oxidation equation. Start by balancing the nitrogen atoms, then balance the oxygen atoms. Adjust the coefficients to ensure the same number of each type of atom on both sides of the equation.

Balance the acetylene oxidation equation. Begin by balancing the carbon atoms, then the hydrogen atoms, and finally the oxygen atoms. Adjust the coefficients to ensure the same number of each type of atom on both sides of the equation.

Verify that both equations are balanced by counting the atoms of each element on both sides of the equations. Ensure that the total number of atoms for each element is equal on the reactant and product sides.

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Key Concepts

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

Balancing Chemical Equations

Balancing chemical equations is essential in chemistry to ensure that the law of conservation of mass is upheld. This means that the number of atoms of each element must be the same on both sides of the equation. To balance an equation, coefficients are adjusted in front of the chemical formulas, allowing for the correct stoichiometric relationships between reactants and products.

Combustion Reactions

Combustion reactions involve the reaction of a substance with oxygen to produce energy, typically in the form of heat and light. For hydrocarbons like acetylene, complete combustion results in carbon dioxide (CO2) and water (H2O) as products. Understanding the stoichiometry of these reactions is crucial for writing balanced equations and predicting the amounts of reactants and products involved.

Oxidation States

Oxidation states (or oxidation numbers) are used to keep track of electron transfer in chemical reactions, particularly in redox reactions. In the context of the question, nitrogen in N2 has an oxidation state of 0, while in N2O5, it has a +5 oxidation state. Recognizing changes in oxidation states helps in understanding the nature of the reaction and the products formed during oxidation.

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Oxidation Numbers

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Textbook Question

Acetylene (C₂H₂) and nitrogen (N₂) both contain a triple bond, but they differ greatly in their chemical properties. (b) By referring to Appendix C, look up the enthalpies of formation of acetylene and nitrogen. Which compound is more stable?

Textbook Question

Acetylene (C₂H₂) and nitrogen (N₂) both contain a triple bond, but they differ greatly in their chemical properties. (d) Calculate the enthalpy of oxidation per mole for N₂ and for C2H₂ (the enthalpy of formation of N₂O₅(g) is 11.30 kJ/mol).

Textbook Question

Acetylene (C₂H₂) and nitrogen (N₂) both contain a triple bond, but they differ greatly in their chemical properties. (e) Both N₂ and C₂H₂ possess triple bonds with quite high bond enthalpies (Table 8.3). Calculate the enthalpy of hydrogenation per mole for both compounds: acetylene plus H₂ to make methane, CH₄; nitrogen plus H₂ to make ammonia, NH₃.

Textbook Question

Under special conditions, sulfur reacts with anhydrous liquid ammonia to form a binary compound of sulfur and nitrogen. The compound is found to consist of 69.6% S and 30.4% N. Measurements of its molecular mass yield a value of 184.3 g/mol. The compound occasionally detonates on being struck or when heated rapidly. The sulfur and nitrogen atoms of the molecule are joined in a ring. All the bonds in the ring are of the same length. (a) Calculate the empirical and molecular formulas for the substance.