Question

\(\mathrm{SiO}_{2}\) is reacted with sodium carbonate. What is the gas liberated? (a) \(\mathrm{O}_{2}\) (b) \(\mathrm{O}_{3}\) (c) CO (d) \(\mathrm{CO}_{2}\)

Short answer

The gas liberated is \(\mathrm{CO}_{2}\).

Step-by-step solution

Understand the Reaction

In this exercise, we are looking at a chemical reaction where silicon dioxide (\(\mathrm{SiO}_2\)) reacts with sodium carbonate (\(\mathrm{Na}_2\mathrm{CO}_3\)). First, it's important to understand that this is a common reaction in industrial processes like glass manufacturing.

Write the Chemical Equation

The reaction can be represented as follows: \[ \mathrm{SiO}_{2} + \mathrm{Na}_{2}\mathrm{CO}_{3} \rightarrow \mathrm{Na}_{2}\mathrm{SiO}_{3} + \mathrm{CO}_{2} \] Here, \(\mathrm{SiO}_{2}\) and \(\mathrm{Na}_{2}\mathrm{CO}_{3}\) react to form sodium silicate (\(\mathrm{Na}_{2}\mathrm{SiO}_{3}\)) and carbon dioxide gas (\(\mathrm{CO}_{2}\)).

Identify the Gas Liberated

From the balanced chemical equation, it is clear that the gas produced or liberated in the reaction is \(\mathrm{CO}_{2}\), carbon dioxide.

Key concepts

Silicon Dioxide

Silicon Dioxide, widely known as silica, is a chemical compound that occurs naturally in several forms, including sand and quartz. It has a chemical formula of \( \mathrm{SiO}_2 \). This compound is a significant material in many industrial processes, especially in the production of glass. When silica is involved in chemical reactions, it often acts as a reactant that undergoes transformation to form new compounds.

In the reaction given, silicon dioxide combines with sodium carbonate to form sodium silicate. This process is not just essential in chemical laboratories but is also widely used in industrial applications such as the production of glass and ceramics. Silica is valued for its properties, like high melting point and strength, which contribute to the stability and durability of final products.

Sodium Carbonate Reaction

Sodium carbonate, or \( \mathrm{Na}_2\mathrm{CO}_3 \), is another key player in chemical reactions and industrial processes. Commonly referred to as soda ash or washing soda, it is a sodium salt of carbonic acid that is often used as a cleaning agent. In chemical reactions, sodium carbonate serves as a source of sodium ions and carbonate ions.

In the reaction with silicon dioxide, sodium carbonate effectively reacts to produce sodium silicate and carbon dioxide. This transformation is vital in glass manufacturing, where it helps to reduce the melting point of the silica, facilitating easier processing. Understanding this reaction allows chemists and industrial engineers to optimize processes for creating various glass types and compositions.

Carbon Dioxide Liberation

The liberation of carbon dioxide \( (\mathrm{CO}_2) \) in chemical processes is a crucial aspect to consider. In the given reaction with silicon dioxide and sodium carbonate, \( \mathrm{CO}_2 \) is produced as a byproduct. This gas is a common product in many reactions involving carbonates and is significant in both natural and industrial contexts.

The release of carbon dioxide in this equation signifies a decomposition of the carbonate ions, which leave the reaction mixture as gas. Managing \( \mathrm{CO}_2 \) emissions is essential, not only for efficiency in reaction processes but also for environmental considerations, as excess \( \mathrm{CO}_2 \) is a greenhouse gas contributing to climate change.

Industrial Processes

Many industrial processes rely on reactions involving silicon dioxide. These include the production of glass, ceramics, and even silicon chips for electronic devices. The specific reaction between \( \mathrm{SiO}_2 \) and \( \mathrm{Na}_2\mathrm{CO}_3 \) to form sodium silicate and carbon dioxide is a primary step in glass-making.

This process helps modify the physical and chemical properties of glass, making it suitable for various applications from windows and bottles to more specialized uses like laboratory glassware. This showcases the intersection of chemistry with real-world applications, emphasizing the importance of understanding chemical reactions in developing and refining industrial processes.

Balanced Chemical Equation

A balanced chemical equation is vital for understanding the specifics of any chemical reaction. In our example, the equation \[ \mathrm{SiO}_2 + \mathrm{Na}_2\mathrm{CO}_3 \rightarrow \mathrm{Na}_2\mathrm{SiO}_3 + \mathrm{CO}_2 \] demonstrates the stoichiometry of the reaction. Each side of the equation has equal numbers of atoms for each element, confirming that mass is conserved.

Balancing chemical equations ensures that the law of conservation of mass is applied, meaning no atoms are lost or gained. This understanding is critical for predicting the quantities of reactants needed and products formed, allowing chemists to design processes efficiently and safely. By grasping how to balance equations, students and professionals alike can better analyze and troubleshoot chemical reactions.