Question

4. The rate of the reaction between hemoglobin (Hb) and carbon monoxide (CO) was studied at 20°C. The following data were collected with all concentration units in umol/L. Note that a hemoglobin concentration of 2.21 umol/L is equal to 2.21 x 10 mol/L. Initial Hb Concentration Initial CO Concentration Initial Rate (umol/L) (umol/L) (umol/L-s) 2.21 1.00 0.619 1.24 4.42 3.00 3.71 3.36 2.40 4.42 100 a. Determine the order of the reaction with respect to hemoglobin and carbon monoxide. b. Determine the rate law. c. Calculate the value of the rate constant. Make sure to include correct units. d. What would the initial rate be for the experiment using the initial concentrations given in the last line of the table?

Answer 1

The rate law is Rate = k [Hb][co] K=rate constant m= order with reapect to Mb n = order with respect to co consider Rowl and Rowl of the table. In these rowe, the co concentration in Kent constant at I umol/L and concentration of Hb is increand twice from 2.21 to 4.42 dimolle Rate law for Rowl il Rate = k[2.215m con 0.619 = K[2.217m cign Rate law for Row 2 in 1.24 = K[4.423m CiJ yo to giver 1.24 Ő Sven 1:24 = K[4-427"03" 0.619 KC2.217m cign k [4.42]mon 2 = qm m=1 of the reaction with respect to & order Hb is m=1 Rate law for row 3 il 321 = K [4.427 "Es* gives 3.71. K[4.423mcja 1-24 K[4-42]m [ign 3= 3n = n=1

order of the reaction with respect to co is n=1 b) The rate law is rate = k [hb][co] © equation 0 in 0.619 = K [2.217M CUJÀ.com umol/2190.619 = k [2-21]' [1]' umolle umo! K = 0.619 emollis 2.21 luomalle umolle K = 0.28 Lumolis (OR) K = 0.28 11156molis = 0.28X106 L moil s' @ Rak = K CHb]m [catm Rate = (0.28creto Lumol.s) (3:36)'(2.40)'umoll, u molle Rate : 2.2579 mmollis