Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

From a thermochemical point of view, explain why a carbon dioxide fire extinguisher or water should not be used on a magnesium fire.

Short Answer

Expert verified
CO₂ and water react with magnesium, making the fire worse.

Step by step solution

01

Understanding Magnesium's Reactivity

Magnesium is a highly reactive metal, especially at higher temperatures. When magnesium is burning, it reacts with various other substances, including oxygen, with a vigorous exothermic reaction that releases a significant amount of heat.
02

Analyzing Carbon Dioxide Reaction with Magnesium

Carbon dioxide (CO₂) is often used in fire extinguishers to smother fires by cutting off the oxygen supply. However, when CO₂ is applied to a magnesium fire, magnesium can continue to burn by reducing CO₂ to carbon (C) and generating an even more exothermic reaction: \( 2Mg + CO_2 \rightarrow 2MgO + C \). This reaction releases heat and intensifies the fire rather than extinguishing it.
03

Examining the Water Reaction with Magnesium

Water (H₂O) should not be used to extinguish a magnesium fire because magnesium reacts vigorously with water. The reaction \( Mg + 2H_2O \rightarrow Mg(OH)_2 + H_2 \) releases hydrogen gas (H₂), which is highly flammable. This could result in an explosion if lit, making the situation more dangerous.
04

Conclusion

Both CO₂ and water react with burning magnesium in a way that can exacerbate the fire. The use of either results in additional reactions that release energy or create flammable gases, hence they are not effective means to extinguish a magnesium fire.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

Key Concepts

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

Magnesium Reactivity
Magnesium is known for its high reactivity, especially when exposed to high temperatures. This metal is a powerhouse in generating enthusiastic and rapid reactions with various elements or compounds. When magnesium burns, it reacts with oxygen in the air, resulting in a vibrant and intense flame. This reaction is called exothermic, meaning it releases heat. Because of this property, magnesium can react explosively with other materials while burning. Understanding this reactivity is crucial, especially in situations where controlling or extinguishing the fire is required.
Carbon Dioxide Reaction
Carbon dioxide (CO₂) is commonly used in fire extinguishers due to its ability to suppress fires by removing oxygen, which is essential for combustion. However, the story changes when it comes to magnesium fires. Instead of putting out the fire, carbon dioxide can participate in a reaction with burning magnesium.
  • The chemical reaction that takes place: \( 2Mg + CO_2 \rightarrow 2MgO + C \)
  • This reaction results in the production of magnesium oxide (MgO) and carbon (C).
  • It releases additional heat, making the situation more explosive.
Using CO₂ will make the fire more intense and difficult to control.
Water Reaction
While water is typically an effective extinguishing agent, it is notably unsuitable for use on magnesium fires. The reaction between water (H₂O) and magnesium is highly vigorous:
  • The reaction follows: \( Mg + 2H_2O \rightarrow Mg(OH)_2 + H_2 \)
  • This produces magnesium hydroxide (Mg(OH)_2) and hydrogen gas (H₂).
  • The release of hydrogen gas is hazardous because it is extremely flammable.
Attempting to extinguish a magnesium fire with water can potentially cause an explosion, significantly increasing the danger of the situation.
Exothermic Reactions
Exothermic reactions are characterized by the release of energy in the form of heat. This principle is at the core of many chemical processes.
  • When a substance burns, there are reactions that release heat and sometimes light.
  • Magnesium, when it reacts with other substances like oxygen, CO₂ , or water, results in exothermic reactions.
  • The energy from these reactions can intensify fires and complicate firefighting efforts.
Understanding exothermic reactions is essential, especially for safety. In magnesium fires, the release of energy not only fuels the ongoing combustion but also catalyzes secondary reactions, which complicate extinguishing efforts.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Determine the enthalpy change for the gaseous reaction of sulfur dioxide with ozone to form sulfur trioxide given the following thermochemical data: $$ \begin{aligned} 2 \mathrm{SO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{2}(g) & \Delta H^{\circ}=-602.8 \mathrm{~kJ} / \mathrm{mol} \\ 3 \mathrm{SO}(g)+2 \mathrm{O}_{3}(g) \longrightarrow 3 \mathrm{SO}_{3}(g) & \\\ \Delta H_{\mathrm{rxn}}^{\circ}=-1485.03 \mathrm{~kJ} / \mathrm{mol} \\ \frac{3}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{O}_{3}(g) & \Delta H_{\mathrm{rxn}}^{\circ}=142.2 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$

Glauber's salt, sodium sulfate decahydrate \(\left(\mathrm{Na}_{2} \mathrm{SO}_{4} .\right.\) \(\left.10 \mathrm{H}_{2} \mathrm{O}\right),\) undergoes a phase transition (i.e., melting or freezing) at a convenient temperature of about \(32^{\circ} \mathrm{C}\) : \(\begin{aligned}{\mathrm{Na}_{2} \mathrm{SO}_{4} \cdot 10 \mathrm{H}_{2} \mathrm{O}(s) \longrightarrow \mathrm{Na}_{2} \mathrm{SO}_{4} \cdot 10 \mathrm{H}_{2} \mathrm{O}(l)}{\Delta H^{\circ}} &=74.4 \mathrm{~kJ} / \mathrm{mol} \end{aligned}\) As a result, this compound is used to regulate the temperature in homes. It is placed in plastic bags in the ceiling of a room. During the day, the endothermic melting process absorbs heat from the surroundings, cooling the room. At night, it gives off heat as it freezes. Calculate the mass of Glauber's salt in kilograms needed to lower the temperature of air in a room by \(8.2^{\circ} \mathrm{C}\). The mass of air in the room is \(605.4 \mathrm{~kg} ;\) the specific heat of air is \(1.2 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}\).

The convention of arbitrarily assigning a zero enthalpy value for the most stable form of each element in the standard state at \(25^{\circ} \mathrm{C}\) is a convenient way of dealing with enthalpies of reactions. Explain why this convention cannot be applied to nuclear reactions.

Metabolic activity in the human body releases approximately \(1.0 \times 10^{4} \mathrm{~kJ}\) of heat per day. Assume that a \(55-\mathrm{kg}\) body has the same specific heat as water; how much would the body temperature rise if it were an isolated system? How much water must the body eliminate as perspiration to maintain the normal body temperature \(\left(98.6^{\circ} \mathrm{F}\right)\) ? Comment on your results. (The heat of vaporization of water is \(2.41 \mathrm{~kJ} / \mathrm{g}\).)

What is the difference between specific heat and heat capacity? What are the units for these two quantities? Which is the intensive property and which is the extensive property?

See all solutions

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free