States of Matter Test - 14

As per the Gay Lussac's law of combining volume of gases, the volumes of gaseous reactants and gaseous products bear a simple whole number ratio with each other if they are measured at same temperature and pressure.
In the reaction $${ N }_{ 2 }+{ 3H }_{ 2 }\longrightarrow { 2H }_{ 3 }$$, ratio by volume of $$N_2,  H_2$$ and $$ NH_3$$ is $$1:3:2$$. This illustrates law of Gay Lussac's law of combining volumes of gases.

Mass of $$1000mL$$ steam = $$1000\times 0.0006=0.6gm$$

KINETIC THEORY OF GASES
(a) All the gases consists of very small molecules or atoms whose volume is negligible compared to volume of container (in case volume of container is very small, then this assumption will be violated)
(b)There is no interaction between gaseous particles (the interaction may appreciably affected under certain conditions of temperature and pressure).
(c)The gaseous molecules are under a continuous state of motion which is unaffected by gravity (the random straight line motion is known as brownian motion)
(d)Due to the continuous motion, collision between gaseous molecules with the wall of container occurs. The collision with the wall of container are responsible for pressure exerted by the gas on the wall of container.
(e)The molecule moves with different speed, however the speed of each molecule keep on changing as the collision occur.
(f)All the collision occurring are considered to be perfectly elastic which implies that there is no loss of energy.
(g)The average kinetic energy of gas will depends on absolute temperature only.

At any given temperature, the vapor pressure of a solution containing a nonvolatile solute is less than that of the pure solvent. This effect is called vapor pressure lowering. The solid line in Figure is a plot of the vapor pressure of pure water versus temperature. The break in the curve at 0°C is the intersection of the curve of the vapor pressure of the solid with the curve of the vapor pressure of the liquid. The dashed line in is a plot of the vapor pressure of an aqueous solution of sugar versus temperature. Notice that the vapor pressure of the solution is always less than that of the pure solvent. 

The vapor pressure of pure water is shown as a solid line; the vapor pressure of an aqueous solution is shown as a dashed line. Note the differences between the solution and the pure substance in melting point and boiling point.

The surface of a pure solvent is populated only by solvent molecules. Some of these molecules are escaping from the surface, and others are returning to the liquid state. The surface of a solution is populated by two kinds of molecules; some are solvent molecules,

Since volume, temperature, and pressure are constant, the number of moles of all the gases will be the same. Hence, the number of molecules of all the gases is also the same. 

Vapour pressure of a dilute solution depends upon the temperature, mole fraction, and degree of dissociation of solute and independent of the melting point of solute.

Avogadro's hypothesis: Equal volume of all gases have equal number of molecules (not atoms) at same temperature and pressures conditions.