Question

Bromine water reacts with \(\mathrm{SO}_{2}\) to form : (1) \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{HBr}\) (2) \(\mathrm{HBr}\) and \(\mathrm{S}\) (3) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and \(\mathrm{HBr}\) (4) \(\mathrm{S}\) and \(\mathrm{H}_{2} \mathrm{O}\) (5) \(\mathrm{Br}_{2}\) and \(\mathrm{SO}_{3}\)

Short answer

Option (3): \(H_2SO_4\) and \(HBr\).

Step-by-step solution

- Understand the Reactants and Products

Bromine water \(Br_2(aq)\) reacts with sulfur dioxide \(SO_2(g)\). We'll need to find the correct combination of products from the given options.

- Write the Balanced Chemical Equation

Write the balanced equation for the reaction: \(Br_2 + SO_2 + 2H_2O \rightarrow 2HBr + H_2SO_4\).

- Identify the Products

From the balanced equation, we can see that the products are \(HBr\) and \(H_2SO_4\).

- Match with Given Options

Check the options to see which one matches the products \(HBr\) and \(H_2SO_4\). The correct option is (3).

Key concepts

Chemical reactions

A chemical reaction is a process where reactants are transformed into products by breaking and forming chemical bonds. In the reaction between bromine water \(\text{Br}_2(aq)\) and sulfur dioxide \(\text{SO}_2(g)\), new substances are created. The original molecules break apart, atoms rearrange, and new bonds form to create different molecules. Understanding how different substances interact and change helps us grasp various chemical concepts and phenomena. In our example, bromine water and sulfur dioxide undergo a chemical reaction to produce specific products.

Balanced equations

Balancing chemical equations is crucial for accurately representing what happens during a reaction. A balanced equation ensures that the number of atoms for each element is conserved throughout the reaction. For our reaction of bromine water and sulfur dioxide, we start with the reactants \(\text{Br}_2\), \(\text{SO}_2\), and \(\text{H}_2\text{O}\). The balanced chemical equation looks like this: \[ \text{Br}_2 + \text{SO}_2 + 2\text{H}_2\text{O} \rightarrow 2\text{HBr} + \text{H}_2\text{SO}_4 \] This equation tells us exactly how many molecules of each reactant combine and how many molecules of each product are formed. It's crucial for predicting how much of each substance is used and produced in the reaction. Balancing equations requires practice but is essential for performing accurate chemical calculations.

Oxidation-reduction reactions

Oxidation-reduction (redox) reactions involve the transfer of electrons between substances. One substance gets oxidized (loses electrons), and another gets reduced (gains electrons). In our given example, the reaction between bromine water and sulfur dioxide is a redox reaction. Bromine \(Br_2\) is reduced to hydrogen bromide \(HBr\), and sulfur dioxide \(SO_2\) is oxidized to sulfuric acid \(H_2SO_4\). Here's how it happens:

• Bromine \(Br_2\) gains electrons and is reduced to \(HBr\).
• Sulfur dioxide \(SO_2\) loses electrons and is oxidized to \(H_2SO_4\).

Recognizing redox reactions helps us understand the flow of electrons, which is fundamental in many chemical processes, including energy production, metabolism, and industrial applications.