Consider the kinetic data given in the following table for the reaction A+B+C\to product Experiment No. [A] (Mol \dm^{-3}) [B] (Mol \dm^{-3}) [C] (Mol \dm^{-3}) Rate of reaction (Mol \dm^{-3}) 1 0.2 0.1 0.1 6.0\times10^{-5} 2 0.2 0.2 0.1 6.0\times10^{-5} 3 0.2 0.1 0.2 1.2\times10^{-4} 4 0.3 0.1 0.1 9.0\times10^{-5} The rate of the reaction for [A]=0.15mol^{-3},[B]=0.25\mol \dm^{-3} and [C]=0.15\mol \dm^{-3} is found to be Y\times10^{-5}. The value of Y is _____ [JEE Adv 2019 P1]

Chemical Kinetics and Nuclear Chemistry

Section: Chemistry

Question : 9 of 33

Marks: +1, -0

Consider the kinetic data given in the following table for the reaction A+B+C→ product

Experiment No.	[A] (Mol dm−3)	[B] (Mol dm−3)	[C] (Mol dm−3)	Rate of reaction (Mol dm−3)
1	0.2	0.1	0.1	6.0×10−5
2	0.2	0.2	0.1	6.0×10−5
3	0.2	0.1	0.2	1.2×10−4
4	0.3	0.1	0.1	9.0×10−5

The rate of the reaction for

[A]=0.15mol−3,[B]=0.25‌mol‌dm−3

and [C]=0.15‌mol‌dm−3 is found to be Y×10−5. The value of Y is _____

[JEE Adv 2019 P1]

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