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

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Chemistry

Nitrogen and oxygen do not react appreciably at roomtemperature, as illustrated by our atmosphere. But at hightemperatures, the reaction below can proceed to a measurableextent. N2(g) + O2(g) ⇔ 2 NO(g) At 3000 K, the reaction above hasKeq = 0.0153. If 0.2702 mol of pure NO is injected into anevacuated 2.0-L container and heated to 3000K, what will be theequilibrium concentration of NO?

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3.7 Ratings (642 Votes)

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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