Chapter 19: Problem 20
What is the gas produced when iron(II) sulfide is treated with a nonoxidizing acid?
Short Answer
Expert verified
The gas produced when iron(II) sulfide is treated with a nonoxidizing acid is hydrogen sulfide (H2S).
Step by step solution
01
Identify the Reaction
When a nonoxidizing acid reacts with iron(II) sulfide (FeS), the acid donates a proton to one of the anions in the compound, which is the sulfide ion (S^(2-)). This leads to the evolution of a gas as a product of the reaction.
02
Write the Chemical Equation
The general chemical equation for the reaction between a nonoxidizing acid, such as hydrochloric acid (HCl), and iron(II) sulfide is: FeS(s) + 2HCl(aq) -> FeCl2(aq) + H2S(g)This shows that the gas produced is hydrogen sulfide (H2S).
03
Identify the Gas Produced
From the chemical equation, we can see that the gas produced from the reaction of iron(II) sulfide with a nonoxidizing acid is hydrogen sulfide (H2S).
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Chemical Reactions
In the context of iron(II) sulfide reacting with a nonoxidizing acid, we delve into the vast landscape of chemical reactions, a fundamental concept in chemistry. Chemical reactions are processes in which substances, known as reactants, transform into different substances called products. This transformation involves the breaking and formation of chemical bonds.
Iron(II) sulfide reacting with a nonoxidizing acid is classified as a double displacement reaction. Here, the iron object is swapped by the acid's hydrogen, leading to the production of iron chloride and hydrogen sulfide gas. As with any chemical reaction, energy is involved; It's either released or absorbed, depending on the nature of the reaction. In this case, the reaction will typically release energy in the form of heat, making it an exothermic process.
Understanding the types of reactions and the energy changes involved helps students grasp the broader implications of chemical reactions in our world, from industrial processes to natural phenomena.
Iron(II) sulfide reacting with a nonoxidizing acid is classified as a double displacement reaction. Here, the iron object is swapped by the acid's hydrogen, leading to the production of iron chloride and hydrogen sulfide gas. As with any chemical reaction, energy is involved; It's either released or absorbed, depending on the nature of the reaction. In this case, the reaction will typically release energy in the form of heat, making it an exothermic process.
Understanding the types of reactions and the energy changes involved helps students grasp the broader implications of chemical reactions in our world, from industrial processes to natural phenomena.
Acid-Base Chemistry
The interaction between iron(II) sulfide and a nonoxidizing acid is an excellent example of acid-base chemistry. In this domain, acids are proton donors, and bases are proton acceptors. Sulfide (S^(2-)), the base in this reaction, accepts protons from the nonoxidizing acid, such as hydrochloric acid (HCl).
When studying acid-base reactions, it's crucial to recognize the role of the solvent, commonly water, in facilitating proton transfer. However, in this case, the solvent is less involved, as the reaction is more about the exchange of ions.
The production of hydrogen sulfide gas in this reaction is an example of how acid-base interactions can lead to the formation of new, sometimes volatile, compounds. Acid-base chemistry is not just a test-tube event; it occurs in many biological systems and environmental processes, underlining its significance in everyday life and in various industries.
When studying acid-base reactions, it's crucial to recognize the role of the solvent, commonly water, in facilitating proton transfer. However, in this case, the solvent is less involved, as the reaction is more about the exchange of ions.
The production of hydrogen sulfide gas in this reaction is an example of how acid-base interactions can lead to the formation of new, sometimes volatile, compounds. Acid-base chemistry is not just a test-tube event; it occurs in many biological systems and environmental processes, underlining its significance in everyday life and in various industries.
Gas Evolution Reactions
Our reaction of interest also fits within the realm of gas evolution reactions, which are chemical reactions that result in the production of a gas. In our scenario, iron(II) sulfide reacts with the nonoxidizing acid to produce hydrogen sulfide gas, a recognizable gas due to its notorious 'rotten egg' smell.
Gas evolution can indicate a reaction has occurred, often visibly through bubbling or change in smell. It is a type of reaction that students can observe easily, making the theoretical concepts more tangible. Gas evolution reactions are essential in various applications, such as manufacturing, environmental science, and even in day-to-day activities like baking.
Grasping the concept of gas evolution reactions ensures a better understanding of reaction dynamics and aids in predicting the outcomes of various chemical interactions.
Gas evolution can indicate a reaction has occurred, often visibly through bubbling or change in smell. It is a type of reaction that students can observe easily, making the theoretical concepts more tangible. Gas evolution reactions are essential in various applications, such as manufacturing, environmental science, and even in day-to-day activities like baking.
Grasping the concept of gas evolution reactions ensures a better understanding of reaction dynamics and aids in predicting the outcomes of various chemical interactions.
Chemical Equation Balancing
An indispensable skill when studying chemical reactions is chemical equation balancing. The chemical equation for our reaction is: \[\text{FeS(s)} + 2\text{HCl(aq)} \rightarrow \text{FeCl}_2(\text{aq}) + \text{H}_2\text{S(g)}\].
Chemical equations must be balanced to obey the law of conservation of mass, which states that matter cannot be created or destroyed. Balancing an equation involves adjusting the coefficients of reactants and products so that the number of atoms for each element is the same on both sides of the equation.
In the given equation, for instance, we have one Fe and one S on both sides, and the two H from HCl combine to make H2, while the two Cl atoms pair up with Fe. Balancing makes equations meaningful and quantitative, enabling stoichiometric calculations that are crucial for tasks ranging from laboratory experiments to industrial-scale chemical production.
Chemical equations must be balanced to obey the law of conservation of mass, which states that matter cannot be created or destroyed. Balancing an equation involves adjusting the coefficients of reactants and products so that the number of atoms for each element is the same on both sides of the equation.
In the given equation, for instance, we have one Fe and one S on both sides, and the two H from HCl combine to make H2, while the two Cl atoms pair up with Fe. Balancing makes equations meaningful and quantitative, enabling stoichiometric calculations that are crucial for tasks ranging from laboratory experiments to industrial-scale chemical production.