For the reaction
(CH3) 3CCl(aq) + OH-(aq) → (CH3) 3COH(aq) + Cl-(aq)
It is found experimentally that doubling the initial concentration of (CH3) 3CCl causes the initial reaction rate to double,but doubling the initial concentration of OH- has no effect on the rate.What is the rate law?
A) Rate = k[(CH3) 3CCl]2[OH-]
B) Rate = k[(CH3) 3CCl][OH-]
C) Rate = k ![For the reaction (CH<sub>3</sub>) <sub>3</sub>CCl(aq) + OH<sup>-</sup>(aq) → (CH<sub>3</sub>) <sub>3</sub>COH(aq) + Cl<sup>-</sup>(aq) It is found experimentally that doubling the initial concentration of (CH<sub>3</sub>) <sub>3</sub>CCl causes the initial reaction rate to double,but doubling the initial concentration of OH<sup>-</sup> has no effect on the rate.What is the rate law? A) Rate = k[(CH<sub>3</sub>) <sub>3</sub>CCl]<sup>2</sup>[OH<sup>-</sup>] B) Rate = k[(CH<sub>3</sub>) <sub>3</sub>CCl][OH<sup>-</sup>] C) Rate = k D) Rate = k[(CH<sub>3</sub>) <sub>3</sub>COH][Cl<sup>-</sup>] E) Rate = k[(CH<sub>3</sub>) <sub>3</sub>CCl]](https://d2lvgg3v3hfg70.cloudfront.net/TB2288/11ea7a3a_9f04_e04c_a82d_1385bfd9350f_TB2288_11.jpg)
D) Rate = k[(CH3) 3COH][Cl-]
E) Rate = k[(CH3) 3CCl]
Correct Answer:
Verified
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