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Dinitrogen tetroxide in its liquid state was used as one of the fuels on the lunar lander for theNASA Apollo missions. In the gas phase it decomposes to gaseous nitrogen dioxide:N2O4(g) ↔ 2NO2(g)Consider an experiment in which gaseous N2O4 was placed in a flask and allowed to reachequilibrium at a temperature where Kp = 0.133. At equilibrium, the pressure of N2O4 wasfound to be 2.71 atm. Calculate the equilibrium pressure of NO2(g).

Answer :

Equilibrium pressure of NO2 (g) is 0.3604. This is calculated from the expression of equilibrium constant.

Dinitrogen tetroxide in its liquid state was used as one of the fuels on the lunar lander. Decomposition of gaseous nitrogen dioxide ,

N2O+ (g)  ---> 2NO2 (g)

chemical equilibrium is the state in which both the reactants and products are present in concentrations which have no further tendency to change with time. For this equilibrium reaction, equilibrium constant can be represented as

K(eq.) = concentration of product / concentration of reactant

In gaseous phase we consider the presence  of the molecule ,

 Kp = [NO2] / [N2O4]

where, Kp = equilibrium constant that equals to 0.133

            [N2O4] = Presence of N2O4 at equilibrium that equals to 2.71.

Putting the values in the expression of equilibrium constant,

0.133 = [NO2]2 / 2.71

[NO2]2 = 0.133 * 2.71

             = 0.3604

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