The reaction shown below occurs in the blood between hemoglobin (hb) and oxygen. hb + o2 ⇄ hbo2which of the following correctly describes this reaction: 1. equilibrium reaction2. in the lungs, the reaction proceeds to the right3. in the muscles, the reaction proceeds to the left4. the k value for the reaction is extremely small. a and d onlyb and c onlya, b, and c onlya, b, c, and d

A, B, C, and D.

Explanation:

The reaction given is reversible, so it's an equilibrium between the left and the right reaction. At some point the velocities of them will be equal, thus statement 1 (or A) is correct.

In the lungs, the oxygen is absorbed and is joined to hemoglobin to be transported, so the reaction proceeds to the formation of HbO2, or for the right, and then statement 2 (or B) is correct.

In the muscles, the oxygen must leave the hemoglobin and then goes to the cells, so the reaction must proceed to the left and the statement 3 (or C) is correct.

The K value is the equilibrium constant for a reversible reaction, which is the multiplication of the concentration of the products elevated by their coefficients divided by the multiplication of the concentration of the reactants multiplied by their coefficients. In this case, K = [HbO2]/([Hb]*[O2]). [O2] must be high, so K has a small value, and statement 4 (or D) is correct.

the temperature of the gas, in k, not celsius.