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Chapter 6: Problem 107

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
A carbon dioxide fire extinguisher or water should not be used on a magnesium fire because the reactions of magnesium with both carbon dioxide and water are exothermic, producing more heat and combustible materials rather than extinguishing the fire. Therefore, using them could intensify the fire instead of extinguishing it.

Step by step solution

01

Understanding the reaction of magnesium with carbon dioxide

Magnesium is a highly reactive metal. When it reacts with carbon dioxide, which is the main component of a carbon dioxide fire extinguisher, rather than extinguishing the fire, it results in a chemical reaction that produces magnesium oxide and elemental carbon. This process is represented by the following balanced chemical equation: \(Mg_{(s)} + CO2_{(g)} 鈫� MgO_{(s)} + C_{(s)}\). This reaction is exothermic, meaning it releases heat, which can potentially feed the fire instead of extinguishing it.
02

Understanding the reaction of magnesium with water

When magnesium comes into contact with water, it reacts vigorously producing magnesium hydroxide and hydrogen gas. This is represented by the following chemical equation: \(Mg_{(s)} + 2H2O_{(l)} 鈫� Mg(OH)2_{(s)} + H2_{(g)}\). This reaction is also exothermic and the hydrogen gas produced can easily catch fire, leading to an even more intense fire.
03

Understanding Fire Extinguishing Principles

The principal mechanism for fire extinguishing usually involves removing heat from the combustion zone or decreasing the concentration of combustible material. Nevertheless, as we have learnt, the reactions of magnesium with both carbon dioxide and water are exothermic and also result in combustible materials. This is why water or a carbon dioxide fire extinguisher should not be used on a magnesium fire as it could make the situation worse by fueling the fire instead of extinguishing it.

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Most popular questions from this chapter

Methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) is an organic solvent and is also used as a fuel in some automobile engines. From the following data, calculate the standard enthalpy of formation of methanol: $$ \begin{aligned} 2 \mathrm{CH}_{3} \mathrm{OH}(l)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(l) \\ \Delta H_{\mathrm{rxn}}^{\circ}=-1452.8 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$

Determine the standard enthalpy of formation of ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) from its standard enthalpy of combustion \((-1367.4 \mathrm{~kJ} / \mathrm{mol})\)

In writing thermochemical equations, why is it important to indicate the physical state (that is, gaseous, liquid, solid, or aqueous) of each substance?

Determine the amount of heat (in \(\mathrm{kJ}\) ) given off when \(1.26 \times 10^{4} \mathrm{~g}\) of ammonia are produced according to the equation $$ \begin{aligned} \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow & 2 \mathrm{NH}_{3}(g) \\\ \Delta H_{\mathrm{rxn}}^{\circ} &=-92.6 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ Assume that the reaction takes place under standardstate conditions at \(25^{\circ} \mathrm{C}\).

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