Select all that apply. The rate law for the reaction 2NO(g) + CU(g) rightarrow 2NOCl(g) is given by R = k[NO][Cl2] If the following is the mechanism for the reaction, NO(g) + Cl2(g) rightarrow NOCl2(g) NOCl2(g) + NO(g) rightarrow 2NOCl(g) which of the following statements accurately describes this reaction? Check all that apply. a. 2nd order reaction b. The first step is the slow step. c. Doubling [NO] would quadruple the rate. d. Cutting [Cl2] in half would decrease the rate by a factor of two. e. The molecularity of the first step is 1. f. Both steps are termolecular.

The statements that accurately describes this reaction are ; ( A and B )

Given that the rate law for the reaction is given as ; R = K[NO] [ Cl₂ ]

and the mechanism for the reaction is expressed as ;

NO(g) + Cl₂(g) > NOCl₂(g)  + NO(g) > 2NOCl(g)

From the rate law R = K[NO] [ Cl₂ ] , the order of the reaction of [ NO ] and [ Cl₂ ]  are both first order respectively therefore when placed together the overall reaction becomes a 2ⁿd order reaction.  while

The first step in the reaction is considered the slow step because it estimates the correct rate law.

Hence in conclusion The statements that accurately describes this reaction are ; 2nd order reaction  and, The first step is the slow step.

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a. 2nd order reaction.  

b. The first step is the slow step.  

Explanation:

r = k[NO][Cl₂]

a. The reaction is first-order in [NO] and first-order in [Cl₂], so it is second-order overall.

b. The first step is the slow step, because it predicts the correct rate law.

c. is wrong. Doubling [NO] would double the rate, because the reaction is first-order in [NO].

d. is wrong. Cutting [Cl₂] in half would halve the rate, because the reaction is first-order in [Cl₂].

e. is wrong. The molecularity is two, because two particles are colliding.

f. is wrong. Both steps are bimolecular.

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