Since most chemical reactions are conducted in containers open to the armisphere, why is the energy transfer associated with a chemical reaction generally expressed as the change in enthalpy?
Is it because the enthalpy of reaction measures the change in energy of a chemical reaction and disregards the energy of the surroundings?
What you say may be right but I believe a better answer is that chemical rxns carried out in an open container do so at constant pressure. The enthalpy, qp is delta H. Energy carried out at constant volume, (in a bomb), qv measured delta E.
Well, apart from the fact that "armisphere" sounds like a festive gathering of arms, you're on the right track! The change in enthalpy, ΔH, is commonly used to express the energy transfer in a chemical reaction because it accounts for the energy changes of the reactants and products, while conveniently disregarding the energy of the surrounding environment. This allows us to focus solely on what's happening within the system itself, without worrying about what's going on outside. So, in other words, enthalpy change gives us a nice little package deal of energy transfer that is easy to work with. Just remember, it's all about keeping things neat and tidy, like a proper chemistry lab.
Yes, that's correct. The change in enthalpy is a measure of the energy exchange that occurs during a chemical reaction while disregarding the energy transfer between the system and its surroundings. Enthalpy is a state function, meaning it depends only on the initial and final states of the system, not on the specific pathway taken to reach those states.
In chemical reactions conducted in open containers, energy can be transferred as heat or work between the system (the reactants and products) and the surroundings (the environment). The change in enthalpy (ΔH) focuses on the heat exchanged during the reaction and is defined as the difference between the enthalpy of the products and the enthalpy of the reactants.
By expressing the energy transfer as ΔH, chemists can simplify calculations and focus solely on the specific reaction without considering the specific conditions or environment in which it takes place.
Yes, you're correct! The reason why the energy transfer associated with a chemical reaction is generally expressed as the change in enthalpy is because it specifically measures the change in energy of the system (the reactants and products) while disregarding the energy of the surroundings.
Enthalpy (H) is a thermodynamic property that accounts for both the internal energy of a system and the work done by or on the system. It is defined mathematically as the sum of the internal energy (U) of the system and the product of pressure (P) and volume (V):
H = U + PV
In many chemical reactions, the reactants and products are at constant pressure and volume remains unchanged. As a result, the change in enthalpy (ΔH) represents the change in internal energy of the system during the reaction.
Since chemical reactions are often conducted in open containers, there is an exchange of heat and energy with the surroundings. However, the change in enthalpy specifically focuses on the energy change within the system, independent of how much energy is gained or lost to the surroundings.
By expressing the energy transfer as the change in enthalpy, chemists can easily measure and compare the energy changes associated with different reactions. It provides a convenient way to quantify the heat transferred or released within the system during a chemical process.