The bromination of acetone that occurs in acid solution is represented by this equation. CH3COCH3(aq) + Br2(aq) → CH3COCH2Br(aq) + Br-(aq) These kinetic data were obtained for given reaction concentrations. Initial concentrations, M CH3COCH3 Br2 H+ 0.30 0.05 0.05 0.30 0.10 0.05 0.30 0.10 0.10 0.40 0.05 0.20 Initial rate, disappearance of Br2, Ms-1 5.7X10-5 5.7X10-5 1.2X10-4 3.1X10-4 Based on these data, the rate equation is 1. Rate = k [CH3COCH3] [H+] 2. Rate = k [CH=COCH3][Br2] 3. Rate = k [CH3COCH3][Br2][H+]2 4. Rate = k [CH3COCH3][Br2][H+] 64% From NCERT NEET - 2008 Subtopic: Definition, Rate Constant, Rate Law | To view explanation, please take trial in the course below. NEET 2023 - Target Batch - Aryan Raj Singh To view explanation, please take trial in the course below. NEET 2023 - Target Batch - Aryan Raj Singh Please attempt this question first. Add Note More Actions
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A reaction is second order with respect to a reactant. How is the rate of rection affected if the concentration of the reactant is
Let the reaction A → B is a 2nd order reaction w.r.t A and conc. of A is ‘a’ mol/L, then rate of reaction can be written as: dxdt=k[A]2 =ka2 (i) When conc. [A] is doubled i.e., [A’] = 2a mol/L Then new rate of reaction d'(x)dt=k[2a]2 = 4ka2 = 4dxdt Thus rate of reaction will become four times where concentration is doubled.
d'(x)dt = ka22 = 14ka2 = 14dxdt The rate of reaction will become one-fourth of the initial rate of reaction. No worries! We‘ve got your back. Try BYJU‘S free classes today!
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