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

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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) â‡” 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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Solution:

Â Â Â Â Â Â Â Â Â Â Â 2 NO(g) â‡” N₂(g) + O₂(g)

Â Â Â Â Â Â Â Â Â Â Â 0.2702Â Â Â Â Â Â Â Â Â 0Â Â Â Â Â Â Â Â Â Â 0 Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â (initial)

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

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

Equilibrium constant for the above reaction can be given as:

K_eq = [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 Â Â Â Â Â Â Â Â Â Â Â Â Â Â [neglecting â€˜xâ€™ since it is very small at the equilibrium]

x² = 19.08

x = 4.36

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