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mr Goodwill [35]
3 years ago
10

Carbonic anhydrase of erythrocytes (Mr 30,000) has one of the highest turnover numbers known. It catalyzes the reversible hydrat

ion of H2O + CO2 ⇄H2CO3 This is an important process in the transport of CO2 from the tissues to the lungs. If 10.0 g of pure carbonic anhydrase catalyzes the hydration of 0.30 g of CO2 in 1 min at 37 C at Vmax, what is the turnover number (kcat ) of carbonic anhydrase (in units of min-1 )?
Chemistry
1 answer:
Afina-wow [57]3 years ago
6 0

Explanation:

According to the given data, the turnover number can be calculated as follows.

      Turnover number = K_{cat} = \frac{V_{max}}{\text{Concentration of enzyme}}

     V_{max} = \frac{\text{Moles of CO_{2} hydrolyzed}{second}

Therefore, moles of CO_{2} hydrolyzed is as follows.

Moles of CO_{2} hydrolyzed = \frac{Mass of CO_{2}}{Molar mass of CO_{2}}

                 = \frac{0.30}{44}

                 = 0.00682 moles

Now, moles of CO_{2} hydolyzed per second is calculated as follows.

Moles of CO_{2} hydolyzed per second = \frac{0.00682}{60}

             = 1.137 \times 10^{-4} moles/second = V_{max}

And,

Moles of enzyme = \frac{Mass}{\text{Molar mass}}

                       = \frac{10.0 \mu g}{30000}

                       = 3.33 \times 10^{-10} moles

Therefore, the value of K_{cat} is as follows.

    K_{cat} = \frac{1.137 \times 10^{-4} moles}{3.333 \times 10^{-10} moles}

               = 0.3411 \times 10^{6} per second

               = 0.3411 \times 60 \times 10^{6} per minute

               = 20.466 \times 10^{6} per minute

Thus, we can conclude that the turnover number (K_{cat}) of carbonic anhydrase (in units of min^{-1}) is 20.466 \times 10^{6} per minute.

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Where Px is the partial pressure of each of the components once equilibrium has been reached and they are expressed in atmospheres. The equilibrium constant Kp depends solely on temperature and is dimensionless.

In the case of the reaction:

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the equilibrium constant Kp is determined by the following expression:

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The system comes to equilibrium at 425 °C, and

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