The sample's volume is affected by the transferring molecules to the vapor phase, underestimating it.
Explanation:
Hello,
Molar properties are said to be measured per unit of mole of the involved substance; more specifically speaking, the molar volume accounts for the volume occupied per mole of the considered substance. In this case, since the affection of the vapor pressure is mean to be explained, we should assume that the experiment is carried out to determine a liquid's molar volume, in such a way, when performing the experiment one must remember that all the liquids have a vapor pressure associated with the pressure exerted by the in-equilibrium molecules of its vapor phase, besides, the vapor pressure causes the liquid to slowly boil as the time go by. In this manner, the vapor pressure could diminish the liquid's molar volume as it is progressively boiled causing an underestimation.
Molar volume is a property of a component in a solution. It is defined as the volume occupied by one mole of the component in the closed system. You would not expect all solutions to execute volume additivity because intermolecular forces between the components come into play. There is no such thing as conservation of volume.
Vapor pressure affects molar volume because gases are very sensitive by these process conditions. Vapor pressure is very temperature-dependent. Consequently, at a different temperature, your component could expand or compress, thus, affecting the molar volume. Moreover, the pressure affects the molecular collisions in the system.
Answer is: both reactions
are exothermic. <span>
In exothermic reactions, heat is released and enthalpy of reaction is less than
zero (as it show second chemical reaction).
According to Le Chatelier's principle when the reaction
is exothermic heat is included as a product (as it show first
chemical reaction).</span>
the reason why Mars is red is because of its regolith, or surface material, contains lots of iron oxide — the same compound that gives blood and rust their hue
