Question

Aluminium carbide on hydrolysis produces methane.

Short answer

Answer: The balanced chemical equation for the reaction between aluminum carbide and water is Al4C3 + 12H2O -> 4Al(OH)3 + 3CH4. The products of this reaction are aluminum hydroxide (Al(OH)3) and methane (CH4).

Step-by-step solution

Write the chemical formulas of the substances involved

We will first write the chemical formulas of the substances involved in the reaction: - Aluminium carbide: Al4C3 - Water: H2O - Methane: CH4

Write the unbalanced chemical equation

Now, we will write the unbalanced chemical equation for the reaction between aluminum carbide and water. Al4C3 + H2O -> Al(OH)3 + CH4

Balance the chemical equation

In order to balance the chemical equation, we need to make sure that the number of atoms of each element on the reactants side is equal to the number of atoms of each element on the products side. Al4C3 + 12H2O -> 4Al(OH)3 + 3CH4 The balanced chemical equation is: Al4C3 + 12H2O -> 4Al(OH)3 + 3CH4

Describe the reaction

Aluminium carbide (Al4C3) reacts with water (H2O) to produce aluminum hydroxide (Al(OH)3) and methane (CH4). In this process, the aluminum atoms in Al4C3 take the hydroxide ions (OH-) from the water molecules, and the carbon atoms in Al4C3 combine with hydrogen atoms from the water molecules to form methane. Overall, the reaction between aluminum carbide and water results in the production of methane gas and the formation of aluminum hydroxide.

Key concepts

Chemical Equations

Understanding chemical equations is essential for studying reactions like the hydrolysis of aluminium carbide to produce methane. A chemical equation represents the transformation of reactants into products through a chemical reaction. It's much like a recipe that describes the ingredients and the result of mixing them in the correct proportions.

For example, in the exercise provided, the initial, unbalanced chemical equation representing the hydrolysis was written as \(Al_4C_3 + H_2O \rightarrow Al(OH)_3 + CH_4\). This equation lists aluminium carbide (\(Al_4C_3\)) and water (\(H_2O\)) as reactants, with aluminium hydroxide (\(Al(OH)_3\)) and methane (\(CH_4\)) as the products. Understanding this equation's components is just the beginning; the true challenge, and a critical skill in chemistry, is balancing it to obey the law of conservation of mass.

Balancing Chemical Reactions

The conservation of mass is a fundamental concept in chemistry, necessitating that all atoms present in the reactants must be accounted for in the products. Balancing chemical reactions involves adjusting the coefficients (the numbers in front of the chemical formulas) to ensure that the number of atoms of each element is equal on both the reactants and products sides of the equation.

In our case, the unbalanced equation \(Al_4C_3 + H_2O \rightarrow Al(OH)_3 + CH_4\) is adjusted to \(Al_4C_3 + 12H_2O \rightarrow 4Al(OH)_3 + 3CH_4\) to balance it. To arrive at this balanced equation, one needs to apply systematic steps, such as counting the number of atoms of each element on both sides and adding coefficients accordingly. This balancing act is not only crucial for academic purposes but also vital in industrial applications, where the amounts of each substance must be accurately measured and used.

Chemical Reaction of Al4C3 with H2O

The chemical reaction involving the hydrolysis of aluminium carbide (\(Al_4C_3\)) with water (\(H_2O\)) is fascinating because it results in the generation of methane gas (\(CH_4\)), a simple hydrocarbon, and aluminium hydroxide (\(Al(OH)_3\)), a compound with various applications.

During this reaction, the water molecules react with aluminium carbide, where the aluminium atoms attract the hydroxidein water (\(OH^-\)), and the carbon atoms bond with the hydrogen atoms from the water, forming methane. This interaction is a showcase of how compounds can be broken down and reassembled into different molecules. The process is exothermic, releasing energy in the form of heat, and it provides a practical method to produce methane for fuel and other uses. It illustrates not only the theoretical aspects of chemistry but also its real-world implications, such as in energy production and material science.