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 1 year ago

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