Applications of chemical equilibria. living systems

applications of chemical equilibria

living systems

living systems

living systems

when the pressure of oxygen gas increases the equilibrium shifts to the right;

when the acidity increases or the pressure of oxygen gas decreases the equilibrium shifts to the left.

living systems

• The protons aid the freeing of oxygen molecules adsorbed on haemin-groups.

• In lungs the reverse process takes place. As a result of the high partial pressure of oxygen gas, the proton isreleased from the haemoglobin. This shifts the dissociation of H2CO3 to the left releasing CO2.

living systems

Carbon monoxide (CO) can adsorb on haemoglobin molecules even better than O2.

living systems

industrial applications

industrial applications

industrial applications

industrial applications

industrial applications

• the synthesis gases enter the vessel, whereupon the pressure increases

• the gases are heated (T increases) • N2 and H2 are passed over a catalyst bed • the partial conversion of N2 and H2 to NH3 takes place • the liberated heat is removed (T and p decrease) • the reaction mixture is further cooled to condense the

ammonia (T and p decrease further) • the ammonia is removed • pressure is exerted on the non-reacted N2 and H2 and

these gases are further used in the production of ammonia.

industrial applications

water purification

water purification

Chlorine gas is normally poorly soluble in water, but it does more than just dissolve as it reacts extremely rapidly with water. This reaction, actually an auto-oxidation reaction, is an equilibrium reaction.

cave equilibria

cave equilibria

Rain-water contains some H2CO3 in addition to other acids. Above-ground and underground the seeping water becomes more and more enriched with CO2, particularly when passing through humus-rich soils. This increases the partial pressure of CO2 in the water.

cave equilibria

kitchen equilibria