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Question

The rate of the reaction between hemoglobin (Hb) and carbon monoxide (CO) was studied at 20oC. The following data were collected with all concentration units μmol/L
(A haemoglobin concentration of 2.21μmol/L is equal to 2.21×106mol/L)
[Hb]0
(μmol/L)
[CO]0
(μmol/L)
Initial rate
(μmolL1S1)
(1) 2.21 1.00 0.619
(2) 4.42 1.00 1.24
(3) 4.42 3.00 3.71
Determine the orders of this reaction with respect to Hb and CO and rate constant.

A
1st order in Hb and Ist order in CO and rate constant is 0.140 L μ mol1s1
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B
1st order in Hb and 1st order in CO and the rate constant is 0.280 L μ mol1s1
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C
1st order in Hb, 2nd order CO and the rate constant is 0.35 L μ mol1s1
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D
2nd order in Hb, 2nd order in CO and the rate constat is 0.24 L μ mol1s1
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Solution

The correct option is C 1st order in Hb and 1st order in CO and the rate constant is 0.280 L μ mol1s1
When the concentration of Hb is doubled and the concentration of CO is kept constant, the rate of the reaction is doubled. Hence, the reaction is first order in [Hb].

When the concentration of CO is tripled and the concentration of Hb is kept constant, the rate of the reaction is tripled. Hence, the reaction is first order in order in [CO].

The rate law expression is r=k[Hb][CO]

Substitute values in the above expression:

0.619=k×2.21×1.00

k=0.280 L μ mol1s1.

Hence, option B is correct.

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