What do all the atomic models have in common?
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The energy required to vaporize 155 g of butane at its boiling point: 61,723 kJ
<h3>Further explanation</h3>Enthalpy is the amount of system heat at constant pressure.
The enthalpy is symbolized by H, while the change in enthalpy is the difference between the final enthalpy and the initial enthalpy symbolized by ΔH.
Delta H reaction (ΔH) is the amount of heat change between the system and its environment
(ΔH) can be positive (endothermic = requires heat) or negative (exothermic = releasing heat)
The standard unit is kilojoules (kJ)
The enthalpy change symbol (ΔH) is usually written behind the reaction equation.
Change in Standard Evaporation Enthalpy (ΔH vap) is a change in enthalpy at the evaporation of 1 mol liquid phase to the gas phase at its boiling point and standard pressure.
Examples of water evaporation:
H₂O (l) ---> H₂O (g); ΔH vap = + 44kJ
The enthalpy of evaporation is positive because its energy is needed to break the attraction between molecules in a liquid
- 155 g of butane
relative molecular mass of butane (C₄H₁₀) = 4.12 + 10.1 = 58 gram / mol
tex]\large{\boxed{mole\:=\:\frac{grams}{relative\:molecular\:mass}}}[/tex]
mole = 2,672
Since the heat of vaporization for butane is 23.1 kj / mol, the energy needed to evaporate 2,672 moles of butane is:
23.1 kJ / mol x 2,672 mol = 61,723 kJ
<h3>Learn more</h3>the heat of vaporization
The latent heat of vaporization
Keywords: the heat of vaporization, butane, mole, gram, exothermic, endothermic
We can describe a positive energetic process as any process which increases the internal energy of the system.
A positive energetic reaction or process is often referred to as being Endothermic. This means that the system which is performing the process absorbs energy. Some examples include:
- Boiling an Egg
- Roasting food over a fire (the food is the reference system)
etc
Therefore, we can confirm that a positive energetic process is one in which the system in question absorbs energy, thus increasing its internal energy.
<em>Since I could not locate the options online, I have provided a general explanation of the concept coupled with a few examples.</em>
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