Carbon monoxide (co) is toxic because it binds more strongly to the iron in hemoglobin (hb) than does oxygen (o2), as indicated by these approximate standard free-energy changes in blood:
reaction a: reaction b: hb+o2hb+co⟶⟶hbo2,hbco, δg∘=−70 kj/mol δg∘=−80 kj/mol
estimate the equilibrium constant k at 298 k for the equilibrium

hbo2+co⇌hbco+o2

Consider the following reaction at equilibrium. 2co2 (g) 2co (g) + o2 (g) h° = -514 kj le châtelier's principle predicts that the equilibrium partial pressure of co (g) can be maximized by carrying out the reaction a. at high temperature and high pressure b. at high temperature and low pressure c. at low temperature and low pressure d. at low temperature and high pressure e. in the presence of solid carbon