Complete and balance each combustion reaction equation: a. C(s) + O2(g) → b. C3H8O(l) + O2(g) → c. CS2(s) + O2(g) → d. C4H6(g) + O2(g) →

Verified step by step guidance

Identify the type of reaction: Combustion reactions involve a substance reacting with oxygen to produce oxides, typically carbon dioxide and water.

For each reaction, write the unbalanced equation with the expected products: a. C(s) + O_2(g) → CO_2(g), b. C_3H_8O(l) + O_2(g) → CO_2(g) + H_2O(g), c. CS_2(s) + O_2(g) → CO_2(g) + SO_2(g), d. C_4H_6(g) + O_2(g) → CO_2(g) + H_2O(g).

Balance the carbon atoms first by ensuring the number of carbon atoms on the reactant side equals the number of carbon atoms in the carbon dioxide on the product side.

Next, balance the hydrogen atoms by adjusting the number of water molecules on the product side to match the hydrogen atoms in the reactants.

Finally, balance the oxygen atoms by adjusting the number of O_2 molecules on the reactant side to match the total number of oxygen atoms needed in the products.

Key Concepts

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

Combustion Reactions

Combustion reactions are chemical processes in which a substance (usually a hydrocarbon) reacts with oxygen to produce carbon dioxide and water, releasing energy. These reactions are typically exothermic, meaning they release heat. Understanding the general form of combustion reactions is essential for balancing the equations correctly.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms of each element is the same on both sides of the equation. This is achieved by adjusting the coefficients of the reactants and products. A balanced equation reflects the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction.

Stoichiometry

Stoichiometry is the quantitative relationship between the reactants and products in a chemical reaction. It allows chemists to calculate the amounts of substances consumed and produced in a reaction based on the balanced equation. Mastery of stoichiometry is crucial for accurately predicting the outcomes of combustion reactions and determining the required amounts of reactants.

Recommended video:

Guided course

01:16

Stoichiometry Concept

Related Practice

Open Question

Consider the balanced equation: 2 N2H4(g) + N2O4(g) → 3 N2(g) + 4 H2O(g). Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms. Mol N2H4 Mol N2O4 Mol N2 Mol H2O 2 _____ _____ _____ _____ 5 _____ _____ _____ _____ _____ 10 _____ _____ 11.8 _____ 2.5 _____ _____ _____ _____ 4.2 _____ _____

Open Question

We prepare a solution by mixing 0.10 L of 0.12 M sodium chloride with 0.23 L of a 0.18 M MgCl2 solution. What volume of a 0.20 M silver nitrate solution is needed to precipitate all the Cl- ions in the solution as AgCl?

Open Question

Consider the unbalanced equation for the combustion of hexane: C6H14(g) + O2(g) → CO2(g) + H2O(g). Balance the equation and determine how many moles of O2 are required to react completely with 7.2 moles of C6H14.