NO 2 reacts with Cl2 gas to form NO 2 Cl:2 NO 2 (g) + Cl2 (g) ® 2 NO 2 Cl (g)The following mechanism has been proposed:NO 2 (g) + Cl2 (g) ® NO 2 Cl (g) + Cl (g) (slow)NO 2 (g) + Cl (g) ® NO 2 Cl (g) (fast)Determine the rate law for the reaction
Question
NO 2 reacts with Cl2 gas to form NO 2 Cl:2 NO 2 (g) + Cl2 (g) ® 2 NO 2 Cl (g)The following mechanism has been proposed:NO 2 (g) + Cl2 (g) ® NO 2 Cl (g) + Cl (g) (slow)NO 2 (g) + Cl (g) ® NO 2 Cl (g) (fast)Determine the rate law for the reaction
Solution
The rate law for a reaction is determined by the slowest (rate-determining) step in the proposed mechanism. In this case, the slow step is:
NO2 (g) + Cl2 (g) → NO2Cl (g) + Cl (g)
The rate law for this step (and thus the overall reaction) is:
Rate = k[NO2][Cl2]
where k is the rate constant, [NO2] is the concentration of NO2, and [Cl2] is the concentration of Cl2. This is because the rate of a reaction is directly proportional to the concentration of the reactants, raised to their stoichiometric coefficients in the rate-determining step. In this case, both coefficients are 1, so the rate law is first order in both NO2 and Cl2.
Similar Questions
A proposed mechanism for the reaction of NO and H 2 gases is given:2NO (g) ⇌ N 2 O 2 (g) fast equilibriumN 2 O 2 (g) + H 2 (g) ® N 2 O (g) + H 2 O (g) slowN 2 O (g) + H 2 (g) ® N 2 (g) + H 2 O (g) fastDerive the rate law for the overall reaction based on the above mechanism.
Given the following balanced equation, determine the rate of reaction with respect to [Cl2]. If the rate of Cl2 loss is 4.00 × 10-2 M/s, what is the rate of formation of NOCl?2 NO(g) + Cl2(g) → 2 NOCl(g)Group of answer choices1.00 × 10-1 M/s4.00 × 10-2 M/s2.00 × 10-2 M/s8.00 × 10-2 M/s7.25 × 10-2 M/s
Write the rate law for the following elementary reaction:CH2CH2(g) + Cl2(g) → CH2CH2Cl+(g) + Cl−(g)Use k1 to stand for the rate constant.
How can you determine the rate law of the following reaction?2NO (g) + O2 (g) → 2NO2 (g)
A chemistry graduate student is studying the rate of this reaction:→2Cl2O5g+2Cl2g5O2gHe fills a reaction vessel with Cl2O5 and measures its concentration as the reaction proceeds:time(seconds) Cl2O50 0.0200M10. 0.0139M20. 0.00966M30. 0.00671M40. 0.00466MUse this data to answer the following questions.Write the rate law for this reaction. rate =k Calculate the value of the rate constant k.Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. =k
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.