(a) Is the dissociation of fluorine molecules into atomic fluorine, F 2 (𝑔) ⇌ 2 F(𝑔), an exothermic or endothermic process?

Hey everyone today, we're being asked if the dissociation of di nitrogen tetroxide into nitrogen gas and oxygen gas is an endo thermic or exotic thermic process, so what does this mean? Exactly? Well, an exotic thermic process, Let's write this in blue. An exotic thermic process, eggs. A thermic process is when heat is released from the reaction heat is released at least and usually results in the formation of bonds or rather is always associated with the formation of bonds. And usually we can see this as when an endo thermic or x atomic reaction takes place. The products are almost always more stable than the reactant and sometimes you can see this in phase changes. So gasses will usually become liquids or become solids. Should the phase change occur in an ex atomic reaction as such because heat is released, the delta H. Of the change in entropy is also negative negative. Endo thermic reactions on the other hand, are the literal opposite. As you might have guessed. Heat is absorbed and breaks bonds. Heat is absorbed bonds break and will usually see the reverse phase change. We can go from solid to liquid to gas. We'll have much more randomness that comes into play bonds break. It will have a positive delta age. So now looking back at the reaction that we have, we have N204 gas becomes into gas And 02 gas so phases aren't changing here, but we have one molecule, we have one molecule becoming two molecules. Right? So the bond in the di nitrogen tetroxide has broken and yields us nitrogen and oxygen gas. So because the bond is breaking, this also means that heat is being absorbed in order to break that bond. Or in other words, this is indeed an endo thermic process. It is endo thermic thermic. I hope this helps, and I look forward to seeing you all in the next one.

Ch.15 - Chemical Equilibrium

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Brown 14th Edition

Ch.15 - Chemical Equilibrium

Problem 69a

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Chapter 15, Problem 69a

(a) Is the dissociation of fluorine molecules into atomic fluorine, F₂(𝑔) ⇌ 2 F(𝑔), an exothermic or endothermic process?

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Identify the type of reaction: The dissociation of fluorine molecules into atomic fluorine is a bond-breaking process.

Recall the general rule that breaking chemical bonds requires energy, while forming chemical bonds releases energy.

Determine the nature of the energy change: Since the reaction involves breaking the F-F bond in F<sub>2</sub>(g) to form atomic fluorine, energy is absorbed from the surroundings.

Conclude the type of thermodynamic process: If a reaction absorbs energy, it is considered endothermic.

State the answer: The dissociation of fluorine molecules into atomic fluorine is an endothermic process.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Dissociation Reactions

Dissociation reactions involve the breaking of bonds in a compound to form individual atoms or smaller molecules. In the case of fluorine, the reaction F₂(g) ⇌ 2 F(g) represents the dissociation of diatomic fluorine into two monatomic fluorine atoms. Understanding this process is crucial for determining the energy changes associated with the reaction.

Exothermic vs. Endothermic Processes

Exothermic processes release energy, usually in the form of heat, while endothermic processes absorb energy from the surroundings. The classification of a reaction as exothermic or endothermic can be determined by the energy changes that occur during bond breaking and formation. This distinction is essential for analyzing the thermodynamics of the dissociation of fluorine.

Bond Energy

Bond energy is the amount of energy required to break a bond between two atoms. In the context of the dissociation of F₂, the bond energy of the F-F bond must be considered to evaluate whether the process is exothermic or endothermic. If the energy required to break the bond is greater than the energy released when forming new bonds, the process is endothermic, and vice versa.

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Bond Energy

Related Practice

Methanol (CH₃OH) can be made by the reaction of CO with H₂: CO(𝑔) + 2 H₂(𝑔) ⇌ CH₃OH(𝑔) (c) To maximize the equilibrium yield of methanol, would you use a high or low pressure?

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Textbook Question

Ozone, O₃, decomposes to molecular oxygen in the stratosphere according to the reaction 2 O31g2¡3 O21g2. Would an increase in pressure favor the formation of ozone or of oxygen?

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Textbook Question

The water–gas shift reaction CO1g2 + H2O1g2Δ CO21g2 + H21g2 is used industrially to produce hydrogen. The reaction enthalpy is H = -41 kJ. (b) Could you increase the equilibrium yield of hydrogen by controlling the pressure of this reaction? If so would high or low pressure favor formation of H2(g)?

(b) If the temperature is raised by 100 K, does the equilibrium constant for this reaction increase or decrease?

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