Sublimation of camphor is exothermic or endothermic

I was doing a laboratory experiment the other day and they asked us to heat a beaker that contained camphor and to cover it with a watch glass with ice on it. I understand the crystallization process and I also know that the melting point of camphor is 149 C, so it is never reached during the experiment, but I do not get the sublimation process. How can the vapor pressure increase until it reaches a value close enough to the atmospheric pressure to sublimate without reaching its melting point? I think I am missing out an important fact, but I don't know which. How can the vapor pressure increase until it reaches a value close enough to the atmospheric pressure to sublimate without reaching its melting point? Compounds can sublimate even if the vapor pressure is much lower than the atmospheric pressure. This is how we can smell solids. If you put the solid substance in a closed container, the partial pressure of the substance in the gas phase will increase until it reaches the vapor pressure, and you will be at equilibrium. In an open system, it will continue to sublimate, with a concentration gradient in the gas phase (that is how the sense of smell is used to locate smelly objects). they asked us to heat a beaker that contained camphor and to cover it with a watch glass with ice on it. In your experimental setup, you never reach an equilibrium. The vapor pressure of the camphor in the beaker is higher than the vapor pressure of the camphor deposited on the cold watch glas...

This input of energy is also enough to overcome the attractive forces that hold the particles together. Water is a good example of a substance that has substantial intermolecular forces holding it together. Water likes to stick to itself though hydrogen bonding. Thus the energy that is input must be enough to have the molecules stop sticking to themselves so much. Riti Gupta holds a Honors Bachelors degree in Biochemistry from the University of Oregon and a PhD in biology from Johns Hopkins University. She has an interest in astrobiology and manned spaceflight. She has over 10 years of biology research experience in academia. She currently teaches classes in biochemistry, biology, biophysics, astrobiology, as well as high school AP Biology and Chemistry test prep.

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Sublimation is a procedure where there is a thermal power alteration in the beginning and ending energy states of the molecules or atoms linked. Several such processes live in physics and chemistry that associate the input or output of thermal energy. If an approach like sublimation releases warmth, it will undoubtedly hail as an exothermic procedure. If the system were to absorb heat, it would be called an endothermic sublimation process. This adjustment in energy state from the start throughout states is associated with the total power scenario of the molecules or atoms, so recognizing whether it is an exothermic or endothermic process offers a researcher an expression of the final energy state. Sublimation Process is Endothermic Or Exothermic Sublimation is the transition of a compound right from the strong to the gas state without travelling through the fluid state. Also, sublimation is an endothermic procedure that shows up at temperatures and stress below a material’s three-way factor in its phase layout, which associates to the lowest pressure at which the material can happen as a liquid. The reverse sublimation process is deposition or desublimation, in which material passes straight from a gas to a solid stage. Sublimation has also been applied as a common term to define a solid-to-gas change (sublimation) pursued by a gas-to-solid transition (deposition). While evaporation from liquid to gas looks like evaporation from the surface if it occurs listed below the li...

https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FIntroductory_Chemistry%2FMap%253A_Fundamentals_of_General_Organic_and_Biological_Chemistry_(McMurry_et_al.)%2F07%253A_Chemical_Reactions_-_Energy_Rates_and_Equilibrium%2F7.03%253A_Exothermic_and_Endothermic_Reactions Expand/collapse global hierarchy • Home • Bookshelves • Introductory, Conceptual, and GOB Chemistry • Map: Fundamentals of General Organic and Biological Chemistry (McMurry et al.) • 7: Chemical Reactions - Energy, Rates, and Equilibrium • 7.3: Exothermic and Endothermic Reactions Expand/collapse global location \( \newcommand\) • • • • • • • • • • Endothermic and Exothermic Reactions Endothermic and exothermic reactions can be thought of as having energy as either a reactant of the reaction or a product. Endothermic reactions require energy, so energy is a reactant. Heat flows from the surroundings to the system (reaction mixture) and the enthalpy of the system increases (\(\Delta H\)is positive). As discussed in the previous section, heat is released (considered a product) in an exothermic reaction, and the enthalpy of the system decreases (\(\Delta H\) is negative). In the course of an endothermic process, the system gains heat from the surroundings and so the temperature of the surroundings decreases (gets cold). A chemical reaction is exothermic if heat is released by the system into the surroundings. Because the surroundings is gaining heat from the ...

Sublimation is an endothermic process. Explain It To A Child Sublimation is a process where a substance changes from a solid to a gas without ever becoming a liquid. When a solid substance goes directly to a gas without passing through the liquid phase, it is called sublimation. The heat absorbed in this process is used to break the intermolecular attractions between the molecules of the solid and turn them into gas molecules. Is sublimation endothermic or exothermic process? Sublimation is an endothermic process. When a substance sublimes, it goes through a phase change from solid to a gas without ever becoming a liquid. This occurs when the particles of the solid gain enough energy to overcome the attractions that are holding them together in a lattice structure. The endothermic nature of sublimation means that heat must be supplied in order to break the attractive forces between particles and cause them to enter the gas phase. In contrast, an exothermic process is one in which heat is released as the reaction occurs. For example, when wood burns, it undergoes an exothermic reaction, releasing heat and light as it is turned into ashes and smoke. Sublimation, on the other hand, is endothermic, meaning that it absorbs heat from its surroundings in order to fuel the reaction. While sublimation can occur at any temperature, it generally happens more quickly at higher temperatures. This is because the hotter a substance gets, the more kinetic energy its particles have and thu...

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Sublimation is a procedure where there is a thermal power alteration in the beginning and ending energy states of the molecules or atoms linked. Several such processes live in physics and chemistry that associate the input or output of thermal energy. If an approach like sublimation releases warmth, it will undoubtedly hail as an exothermic procedure. If the system were to absorb heat, it would be called an endothermic sublimation process. This adjustment in energy state from the start throughout states is associated with the total power scenario of the molecules or atoms, so recognizing whether it is an exothermic or endothermic process offers a researcher an expression of the final energy state. Sublimation Process is Endothermic Or Exothermic Sublimation is the transition of a compound right from the strong to the gas state without travelling through the fluid state. Also, sublimation is an endothermic procedure that shows up at temperatures and stress below a material’s three-way factor in its phase layout, which associates to the lowest pressure at which the material can happen as a liquid. The reverse sublimation process is deposition or desublimation, in which material passes straight from a gas to a solid stage. Sublimation has also been applied as a common term to define a solid-to-gas change (sublimation) pursued by a gas-to-solid transition (deposition). While evaporation from liquid to gas looks like evaporation from the surface if it occurs listed below the li...

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https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FIntroductory_Chemistry%2FMap%253A_Fundamentals_of_General_Organic_and_Biological_Chemistry_(McMurry_et_al.)%2F07%253A_Chemical_Reactions_-_Energy_Rates_and_Equilibrium%2F7.03%253A_Exothermic_and_Endothermic_Reactions Expand/collapse global hierarchy • Home • Bookshelves • Introductory, Conceptual, and GOB Chemistry • Map: Fundamentals of General Organic and Biological Chemistry (McMurry et al.) • 7: Chemical Reactions - Energy, Rates, and Equilibrium • 7.3: Exothermic and Endothermic Reactions Expand/collapse global location \( \newcommand\) • • • • • • • • • • Endothermic and Exothermic Reactions Endothermic and exothermic reactions can be thought of as having energy as either a reactant of the reaction or a product. Endothermic reactions require energy, so energy is a reactant. Heat flows from the surroundings to the system (reaction mixture) and the enthalpy of the system increases (\(\Delta H\)is positive). As discussed in the previous section, heat is released (considered a product) in an exothermic reaction, and the enthalpy of the system decreases (\(\Delta H\) is negative). In the course of an endothermic process, the system gains heat from the surroundings and so the temperature of the surroundings decreases (gets cold). A chemical reaction is exothermic if heat is released by the system into the surroundings. Because the surroundings is gaining heat from the ...