The reaction is
N₂O₄(g) <=> 2NO₂(g)
a. Initial pressure is 5.3 atm
We assume that the there is 1 mole at the start
N₂O₄(g) <=> 2NO₂(g)
1
-x 2x
---------------------------
1 - x 2x
The total moles is
1 + x
The mole fraction of N2O4 is
(1 - x)/(1 + x)
The mole fraction of NO2
2x/(1 + x)
Kp = [2x/(1 + x)]² / [(1 - x)/(1 + x)] = 0.25
Solve for x
And the total number of moles
The total pressure is solved by
(1 + x) (5.3)
The partial pressure of N2O4 is
5.3 (1 - x)
The partial pressure of NO4 is
5.3 (2x)
Do the same for the second problem.
The answer to this item is the first choice, MOLECULES. The molecules are the smallest particles of both the compounds and even the biatomic elements. They are made up of atoms that are being held together through chemical bonds of different types depending on the type of atoms that shared the electrons.
There are 2 types of electricity, static electricity and current electricity
M (C2H6) = n × M = 4.6 × 30 = 13.8 g.
