1. (5pts) The reaction: CH3CHCH2(g) + HCl(g) -＞ CH3CHClCH3(g) and the possible mechanism is 2 HCl ⇌ (HCl)2 (Fast equilibrium) CH3CHCH2 + HCl ⇌ complex (Fast equilibrium) Complex + (HCl)2 -＞ CH3CHClCH3 + 2HCl (Slow equilibrium) Derive the rate law for this reaction using this mechanism.

3. (5pts) Consider the system: A(g) -＞ B(g) at 25°C. a. (3pts) Assuming that G°A = 8996 J/mol and G°B = 11,718 J/mol, calculate the value of the equilibrium constant for this reaction. b. (2pts) Calculate the equilibrium pressure that result if 1.00 mole of A(g) at 1.00 atm and 1.00 mole of B(g) at 1.00 atm are mixed at 25°C. (e^1.1 = 3.0, e^2.1 = 8.2)

1. (5pts) The reaction: CH3CHCH2(g) + HCl(g) -＞ CH3CHClCH3(g) and the possible mechanism is 2 HCl ⇌ (HCl)2 (Fast equilibrium) CH3CHCH2 + HCl ⇌ complex (Fast equilibrium) Complex + (HCl)2 -＞ CH3CHClCH3 + 2HCl (Slow equilibrium) Derive the rate law for this reaction using this mechanism.

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