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Following data is given for the reaction,X+YP

Experiment[X] mol L1[Y] mol L1Initial rate mol L1s1
I2.5×10-46×10-55×10-4
II5×10-412×10-54×10-3
III1×10-312×10-51.6×10-2

The order of reaction with respect to X and Y respectively are

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a
1 and 2
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2 and 1
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1 and 1
d
2 and 2

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detailed solution

Correct option is B

Let the order of reaction with respect ta X and Y be a and b, the rate law expression r=k[X]a[Y]bSimilarly,  Exp. I. 5×10−4=k2.5×10−4a6×10−5b            ………(i)                 Exp. II. 4×10−3=k5×10−4a12×10−5b            ………(ii)                 Exp. III. 1.6×10−2=k1×10−3a12×10−5b       ………(iii)From Eqs. (i) and (ii),            4×10−35×10−4=5×10−42.5×10−4a12×10−56×10−5b                                           8=(2)a(2)b                                         ……..(iv)From Eq. (ii) and (iii),            1.6×10−24×10−3=1×10−35×10−4a12×10−512×10−5b                             4=(2)a(2)2=(2)a                          ∴ a=2       On substituting value of a in Eq. (iv), we get                                    8=(2)2(2)b                                 (2)=(2)b or b=1Thus, order of reaction with respect ta X is 2 and with respect to Y is 1.

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Similar Questions

For the non-stoichiometric reaction 2A+BC+D, the following kinetic data were obtained in three separate experiments, all at 298 K.

Initial
concentration [A]
Initial
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0.1 M0.1 M1.2×10-3
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The rate law for the formation of C is


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