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Chapter 17: Problem 6

When sodium bicarbonate is heated, the product obtained is (a) \(\mathrm{Na}\) (b) \(\mathrm{NaCO}_{3}\) (c) \(\mathrm{NaHCO}_{3}\) (d) \(\mathrm{Na}_{2} \mathrm{CO}_{3}\)

Short Answer

Expert verified
The product is (d) \(\mathrm{Na}_{2} \mathrm{CO}_{3}\).

Step by step solution

01

Understand the Decomposition Reaction

Sodium bicarbonate (NaHCO鈧�) decomposes when heated. This is a common chemical reaction where a bicarbonate compound breaks down to form a metal carbonate, water, and carbon dioxide. The reaction can be expressed as: \(2 \mathrm{NaHCO}_{3} \rightarrow \mathrm{Na}_{2} \mathrm{CO}_{3} + \mathrm{H}_{2}\mathrm{O} + \mathrm{CO}_{2}\).
02

Identify the Products of the Reaction

According to the decomposition equation, heating sodium bicarbonate produces sodium carbonate (Na鈧侰O鈧�), along with water (H鈧侽) and carbon dioxide (CO鈧�). The focus in the options given is on the solid compound formed, which is sodium carbonate (Na鈧侰O鈧�).
03

Match the Product with Given Options

Among the given options (a) Na, (b) NaCO鈧�, (c) NaHCO鈧�, and (d) Na鈧侰O鈧�, the compound that matches the expected product (sodium carbonate) from the decomposition is option (d) Na鈧侰O鈧�.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Sodium Carbonate Formation
Sodium carbonate, also known as soda ash or washing soda, is formed when sodium bicarbonate is heated. This reaction is a classic example of a thermal decomposition process. When you heat sodium bicarbonate ( NaHCO鈧�), it breaks down into three products: sodium carbonate ( Na鈧侰O鈧�), water ( H鈧侽), and carbon dioxide ( CO鈧�).
  • Heat causes the bicarbonate to lose a molecule of carbon dioxide and water, leaving behind sodium carbonate.
  • The resulting sodium carbonate remains as a solid, which makes this reaction very useful in various applications such as glass manufacturing and in laundry detergents.
The importance of this reaction lies in obtaining sodium carbonate from the easily available and inexpensive sodium bicarbonate. Remember, sodium carbonate is more stable at higher temperatures compared to bicarbonate, making it a crucial compound in industrial processes.
Thermal Decomposition
Thermal decomposition is a type of chemical reaction where a compound breaks down into simpler substances when heat is applied. In the case of sodium bicarbonate, the decomposition occurs as the bicarbonate heats up.
  • The process involves breaking chemical bonds in the sodium bicarbonate molecules, which requires energy in the form of heat.
  • This energy input allows the bicarbonate ions to separate, releasing carbon dioxide gas and forming liquid water.
The thermal decomposition reaction of sodium bicarbonate is endothermic, meaning it absorbs heat from the surroundings. This is in contrast with exothermic reactions, which release heat.
Understanding thermal decomposition is crucial as it applies to numerous other chemical reactions and industries, beyond just the heating of sodium bicarbonate.
Bicarbonate Reactions
Bicarbonate reactions, such as the decomposition of sodium bicarbonate, are part of a broader class of chemical reactions involving bicarbonate ions ( HCO鈧冣伝).
  • Bicarbonates are typically formed from the reaction between a base, such as sodium hydroxide, and carbonic acid.
  • These reactions are reversible, meaning bicarbonates can decompose back into carbon dioxide and the original hydroxide compound.
In everyday life, bicarbonate reactions are essential. For example, the reaction of baking soda, a common bicarbonate, with acids like vinegar is widely used in cooking as a leavening agent. It helps dough rise by releasing carbon dioxide gas, which expands within the dough.
Understanding bicarbonate reactions extends to environmental science as well. In water bodies, bicarbonates play a role in maintaining pH balance as they react in equilibrium with carbon dioxide and carbonate.

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Most popular questions from this chapter

Which of the following reactions written here are correct? (1) \(\mathrm{B}+\mathrm{NaOH} \longrightarrow 2 \mathrm{Na}_{3} \mathrm{BO}_{3}+\mathrm{H}_{2}\) (2) \(\mathrm{P}_{4}+\mathrm{NaOH}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{NaH}_{2} \mathrm{PO}_{2}+\mathrm{PH}_{3}\) (3) \(\mathrm{S}+\mathrm{NaOH} \longrightarrow \mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}+\mathrm{Na}_{2} \mathrm{~S}+\mathrm{H}_{2} \mathrm{O}\) (a) 1 only (b) 3 only (c) 2 and 3 (d) 1,2 and 3

Which of the following carbonates cannot evolve \(\mathrm{CO}_{2}\) on heating? (a) \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) (b) \(\mathrm{Rb}_{2} \mathrm{CO}_{3}\) (c) \(\mathrm{Li}_{2} \mathrm{CO}_{3}\) (d) \(\mathrm{MgCO}_{3}\)

In the reaction: \(\mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]+\mathrm{K}_{2} \mathrm{CO}_{3} \longrightarrow\) the product formed is (a) \(\mathrm{FeCO}_{3}\) (b) \(\mathrm{KCN}\) (c) \(\mathrm{KFeCO}_{3}\) (d) \(\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{4}\right]\)

Which of the following set of raw materials are used in the manufacture of \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) by Solvay process? (a) \(\mathrm{CaCl}_{2}, \mathrm{NH}_{3}, \mathrm{CO}_{2}\) (b) \(\mathrm{NaOH}, \mathrm{NH}_{3}, \mathrm{CO}_{2}\) (c) \(\mathrm{NaCl}, \mathrm{NH}_{3}, \mathrm{CO}_{2}\) (d) \(\mathrm{Ca}(\mathrm{OH})_{2}, \mathrm{NH}_{3}, \mathrm{CO}_{2}\)

Fluorosis disease is caused due to the reaction of \(\ldots \ldots\). with excess of fluoride in the body. (a) \(\mathrm{Mg}\) (b) \(\mathrm{Fe}\) (c) \(\mathrm{K}\) (d) \(\mathrm{Ca}\)
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