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The equilibrium constant, K, for binding of haemoglobin for carbon monoxide, CO, is about 200-300 times...

The equilibrium constant, K, for binding of haemoglobin for carbon monoxide, CO, is about 200-300 times greater than for O2. Explain using chemical equilibrium principles why this makes breathing CO hazardous.

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Ans.

#I. Reaction 1:           Hb + CO <------> Hb- CO

            Keq1 = [Hb- CO] / ([Hb] [CO])

#II. Reaction 2:         Hb + O2 <------> Hb-O2

            Keq2 = [Hb-O2] / ([Hb] [O2])

# Comparing the two equilibrium constants –

            Keq1 / Keq2 = {[Hb- CO] / ([Hb] [CO])} / {[Hb-O2] / ([Hb] [O2])}

            Or, X = [Hb- CO] [O2] / ([Hb-O2] [CO])

            Or, X = ([Hb- CO] / [Hb-O2]) ([O2] / [CO])

Where, X is the ration (Keq1 / Keq2)

# Given, (Keq1 / Keq2) is around 200- 300.

The following explanations can be presented-

1. X = ([Hb- CO] / [Hb-O2]) when ([O2] / [CO]) = 1. When [CO] is equal to [O2] (say, when some inhales smoke), the [Hb-CO] is around 200-300 times that of [Hb-O2]. Therefore, the equilibrium shifts towards formation of carboxyhemoglobin (Hb-CO). In such case, Hb can’t bind O2 at significant rates, thus drastically limiting O2 supply to the body parts.

Therefore, inhaling CO can deprive the body from oxygenation which may further lead to death due to inhibition of cellular respiration pathways.

queen_honey_blossom answered 2 years ago
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