Question

Given, \[1\] mole of $N_2$​ and $3$ moles of \[{H_2}\] ​are mixed in \[8.21\] lit. container at \[300\] K to form \[N{H_3}\]​ .If on equilibrium average molecular mass was found to be \[34/3\] gram then find partial pressure of \[N{H_3}\] component.

Answer 1

Hint: In an aggregate of gases, every constituent fueloline has a partial strain that is the notional strain of that constituent fueloline if it by myself occupied the complete quantity of the unique aggregate on the identical temperature.[The general strain of a perfect fueloline aggregate is the sum of the partial pressures of the gases withinside the aggregate (Dalton's Law).

Complete Answer:
The partial strain of a fueloline is a degree of thermodynamic interest of the fueloline's molecules. Gases dissolve, diffuse, and react in step with their partial pressures, and now no longer in step with their concentrations in fuel line combos or liquids. This well-known belongings of gases is likewise genuine in chemical reactions of gases in biology. For example, the vital quantity of oxygen for human respiration, and the quantity this is toxic, is ready via means of the partial strain of oxygen by myself. This is genuine throughout a totally huge variety of various concentrations of oxygen found in numerous inhaled respiratory gases or dissolved in blood.

Initially: \[1\] $3$ $0$
                                   \[28\] \[6\]g
At Equilibrium: \[(1 - x)\] \[(3 - 3x)\] \[\;\;(2x)\]
Total moles at equilibrium= \[1 - x + 3 - 3x + 2x = {\text{ }}4 - 2x\]
Average molecular mass= \[\dfrac{{28 + 6}}{{4 - 2x}} = \dfrac{{34}}{3}\]
\[x = 0.5\]

\[0.5\] \[\;1.5\] \[1\]
\[{N_{total}}\]= $3$
\[{P_{total}}\]= \[P{N_2} + {\text{ P}}{H_2} + PN{H_3}\]
= \[\dfrac{{{n_{total}}RT}}{V}\]
=\[\dfrac{{3 \times 0.0821 \times 300}}{{8.21}} = 9\]
P\[{N_2}\]= \[\dfrac{{0.5}}{3} \times 9 = 1.5\]
P\[N{H_3}\]= \[\dfrac{1}{3} \times 9 = 3\]
P\[{H_2}\]= \[\dfrac{{1.5}}{3} \times 9 = 4.5\]

Note:
Dalton's regulation expresses the reality that the entire strain of a combination of perfect gases is identical to the sum of the partial pressures of the person gases within side the combination. This equality arises from the reality that during a really perfect fueloline the molecules are up to now aside that they do now no longer engage with every other. Most real real-international gases come very near this perfect.