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 |
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NEET 2023 - Target Batch - Aryan Raj Singh
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NEET 2023 - Target Batch - Aryan Raj Singh
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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
(i) Doubled
(ii) Reduced to 1/2?
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.
(ii) Similarly, when conc. of A is reduced to 12 i.e., [A] is a/2 then new rate of reaction,
d'(x)dt = ka22 = 14ka2 = 14dxdt
The rate of reaction will become one-fourth of the initial rate of reaction.
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