2 g CO g Cl 2 CO g is rate of reaction k Cl 2 3 2 CO Show that the following

# 2 g co g cl 2 co g is rate of reaction k cl 2 3 2 co

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2 ( g ) + CO ( g ) Cl 2 CO ( g ) is rate of reaction = k [ Cl 2 ] 3 / 2 [ CO ] Show that the following mechanism is consistent with this rate law. (1) Cl 2 (g) k 1 -- * ) -- k – 1 2 Cl(g) (fast equilibrium) (2) Cl(g) + CO(g) k 2 -- * ) -- k – 2 ClCO (g) (fast equilibrium) (3) ClCO (g) + Cl 2 (g) k 3 --→ Cl 2 CO (g) + Cl (g) (slow) Express k in terms of the rate constants for the individual steps of the reaction mech- anism. (b) An alternative mechanism for the chemical reaction in part (a) is (1) Cl 2 (g) k 1 -- * ) -- k – 1 2 Cl (g) (fast equilibrium) (2) Cl (g) + Cl 2 (g) k 2 -- * ) -- k – 2 Cl 3 (g) (fast equilibrium) (3) Cl 3 (g) + CO (g) k 3 --→ Cl 2 CO (g) + Cl (g) (slow) Show that this mechanism also gives the observed rate law. How would you go about determining whether this mechanism or the previous one is correct?
5. [McQuarrie 18-6] Cryosurgical procedures involve lowering the body temperature of the patient prior to surgery. Given that the activation energy for the beating of the heart muscle is about 30kJ, estimate the pulse rate at 22 C. Assume the pulse rate at 37 C (body temperature) to be 75 beats/min. 6. [McQuarrie 18-47] Some reactions have an activation energy, E a = 0. What would the rate of such a reaction depend on? 7. [McQuarrie 18-5] The denaturation of a certain virus is a first-order process with an activation energy of 586 kJ/mol. The half-life of the reaction at 29.6 C is 4.5 hours. Calculate the half-life at 37.0 C.

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