Question

In: Chemistry

Nitrogen and oxygen do not react appreciably at room temperature, as illustrated by our atmosphere. But...

Nitrogen and oxygen do not react appreciably at room temperature, as illustrated by our atmosphere. But at high temperatures, the reaction below can proceed to a measurable extent. N2(g) + O2(g) ⇔ 2 NO(g) At 3000 K, the reaction above has Keq = 0.0153. If 0.2702 mol of pure NO is injected into an evacuated 2.0-L container and heated to 3000K, what will be the equilibrium concentration of NO?

Solutions

Expert Solution

Solution:

            2 NO(g) ⇔ N2(g) + O2(g)

            0.2702          0           0                        (initial)

(0.2702-x)      0.5x       0.5x                             (Equilibrium, moles)

            (0.2702-x)/2      0.5x/2       0.5x/2       (Equilibrium, moles/L)

Equilibrium constant for the above reaction can be given as:

Keq = [N2][O2]/ [NO]2 = 1/0.0153

(0.5x/2)( 0.5x/2)/ [(0.2702-x)/2]2 = 65.35

0.25x2 / (0.2702-x)2 = 65.35

0.25x2 = 4.77                [neglecting ‘x’ since it is very small at the equilibrium]

x2 = 19.08

x = 4.36


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