Question

Apply The general form of a chemical reaction is \(x A+y B \rightarrow z A B\) . In the equation, A and \(B\) are elements, and \(x, y,\) and \(z\) are coefficients. State the mole ratios for this reaction.

Short answer

For the general form of a chemical reaction \(x A + y B \rightarrow z AB\), the mole ratios are: 1. A:B which is \(\frac{x}{y}\) 2. A:AB which is \(\frac{x}{z}\) 3. B:AB which is \(\frac{y}{z}\)

Step-by-step solution

Identify the coefficients

In the given chemical reaction \(x A + y B \rightarrow z AB\), the coefficients for elements A, B, and the compound AB are x, y, and z, respectively.

Write the mole ratios for each element and compound

The mole ratios are written based on the coefficients of each reactant and product in the balanced chemical equation. We can write the mole ratios as: 1. Mole ratio of A to B: \(\frac{x}{y}\) 2. Mole ratio of A to AB: \(\frac{x}{z}\) 3. Mole ratio of B to AB: \(\frac{y}{z}\)

Report the mole ratios for the given reaction

For the general form of a chemical reaction \(x A + y B \rightarrow z AB\), the mole ratios are: 1. A:B which is \(\frac{x}{y}\) 2. A:AB which is \(\frac{x}{z}\) 3. B:AB which is \(\frac{y}{z}\)

Key concepts

Chemical Reactions

Chemical reactions are processes by which substances, called reactants, are transformed into different substances, known as products. In the simplest terms, they are exchanges at the atomic or molecular level resulting in the formation of new compounds. This process is essential in chemistry and occurs in many forms, from combustion to oxidation.
When engaging with a chemical reaction, it's vital to understand:

• Reactants: These are the starting substances that undergo the change.
• Products: These are the new substances formed as a result of the reaction.
• Reaction Medium: The environment in which the reaction takes place, which can affect the rate and outcome.
• Energy Changes: Reactions can be exothermic (release energy) or endothermic (absorb energy).

Chemical reactions often require specific conditions to proceed, such as temperature, pressure, or the presence of a catalyst. The fundamental principle is that matter is neither created nor destroyed, aligning with the law of conservation of mass, which states that the mass of the products must equal the mass of the reactants.

Mole Ratios

In stoichiometry, mole ratios are critical for understanding the quantitative relationships in a chemical reaction. A mole ratio is a conversion factor derived from the coefficients of a balanced chemical equation, representing how much of one substance reacts or is produced relative to another.
For example, if a chemical reaction is given as:
\[ xA + yB \rightarrow zAB \]
The mole ratio helps us understand the following:

• The Ratio Between Reactants:
  • Mole ratio of A to B: \(\frac{x}{y}\)
• The Ratio Between Reactant and Product:
  • Mole ratio of A to AB: \(\frac{x}{z}\)
  • Mole ratio of B to AB: \(\frac{y}{z}\)

These ratios are essential for calculating:

• The amount of reactants needed.
• The quantity of products formed.
• Yield and efficiency of the reaction.

Understanding mole ratios allows precise predictions of how much of each substance is involved or final amounts of products formed in a chemical reaction.

Balanced Equations

Balanced chemical equations are vital because they ensure compliance with the law of conservation of mass. This law states that matter cannot be created or destroyed in a chemical reaction.
To balance a chemical equation, you adjust the coefficients (numbers in front of the chemical formulas) to ensure that the number of each type of atom is the same on both sides of the equation.

• Start by writing the unbalanced equation with the correct chemical formulas for each reactant and product.
• List all elements involved and count the number of atoms for each one in both reactants and products.
• Adjust coefficients to achieve balance, beginning with the most complex molecule or the element appearing in the fewest substances.
• Check your work to ensure that all atoms balance and the coefficients are in the simplest ratio.

Balanced equations are necessary for various chemical calculations, particularly in predicting the amounts of products that will form from certain reactants using mole ratios. When a balanced equation is in place, it allows for precise stoichiometric calculations that are crucial for laboratory and industrial chemical processes.