Is no2(g)+co(g)→no(g)+co2(g) an elementary reaction? Rate = k[NO2]^2 Please explain if possible why It is or...
Is no2(g)+co(g)→no(g)+co2(g) an elementary reaction? Rate = k[NO2]^2
Please explain if possible why It is or is not an elementary reaction
Homework Answers
For elementary reaction, corresponding stoichiometry is only the order of the reaction with respect to that reactant. So, as in the reaction, stoichiometry of NO2 is 1 but according to the given rate law the order the reaction w.r.t to NO2 is 2. Therefore, the reaction stated is not elementary reaction.
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Is no2(g)+co(g)→no(g)+co2(g) an elementary reaction? Rate =
k[NO2]^2
Please explain if possible why It is or...
If the mechanism behind the reaction NO2(g) + CO(g) Ó NO(g) + CO2(g) is : 1-...
If the mechanism behind the reaction NO2(g) + CO(g) Ó NO(g) + CO2(g) is : 1- 2NO2(g) à 2NO(g) + O2(g) (slow) 2- NO(g) + CO(g) + O2(g) à NO2(g) + CO2(g) (fast) Then its rate law is: A) Rate = k [NO2] . [CO] B) Rate = k [NO2] . [CO2] C) Rate = k [NO 212 D) Rate = k [co]2
The reaction rate of CO and NO2 in the reaction CO(g) + NO2(g) → CO2(g) +...
The reaction rate of CO and NO2 in the reaction CO(g) + NO2(g) → CO2(g) + NO(g) is measured using the initial rates method. The results are tabulated below. [CO] (mol/L) NO2 (mol/L) -([CO]/Δt (mol/L·s) 8.00 10-4 5.50 10-4 8.40 10-8 8.00 10-4 7.78 10-4 1.68 10-7 1.60 10-3 5.50 10-4 1.68 10-7 Determine the rate expression and calculate the rate constant for the reaction.
The rate of the reaction: CO (g) + NO2 (g) à CO2 (g) + NO (g)...
The rate of the reaction: CO (g) + NO2 (g) à CO2 (g) + NO (g) was measured at several temperatures, and the following data were collected: Temp (oC) K (M-1s-1) 35 0.184 45 0.322 Using this data determine the value of Ea (energy of activation)
The rate of the reaction: NO2(g) + CO(g) → NO(g) + CO2(g) was determined in three...
The rate of the reaction: NO2(g) + CO(g) → NO(g) + CO2(g) was determined in three experiments at 225°C. The results are given in the following table: Experiment NO2(M) CO (M) Initial Rate –ΔNO2/Δt (M/s) 1 0.277 0.898 0.19 2 0.277 0.449 0.19 3 0.462 0.449 0.576 Calculate the value of the rate constant at 225°C using reaction 1 data
For the reaction NO2(g) + CO(g) → NO(g) + CO2(g)
For the reaction NO2(g) + CO(g) → NO(g) + CO2(g) calculate the order of the reaction with respect to the following reactants according to the following experimental data: Part 1 (1 point) Order of the reaction with respect to NO2: Part 2 (1 point) Order of the reaction with respect to CO:
6. The rate law for the following reaction is rate=k[NO2] (F2]: 2NO2(g) + F2(g) → 2NO2F(g)...
6. The rate law for the following reaction is rate=k[NO2] (F2]: 2NO2(g) + F2(g) → 2NO2F(g) The mechanism proposed for this reaction is as follows: (i) NO2(g) + F2(g) → NO2F(g) + F(g) (ii) NO2(g) + F(g) → NO2F(g) Which elementary step is the rate-determining step in this reaction? Explain your answer in 1-2 sentences.
The reaction NO2(g) + CO(g) CO2(g) + NO(g) has a rate constant of 2.57 M−1∙s−1 at...
The reaction NO2(g) + CO(g) CO2(g) + NO(g) has a rate constant of 2.57 M−1∙s−1 at 701 K and 567 M−1∙s−1 at 895 K. Find the activation energy in kJ/mol
To understand how elementary steps make up a mechanism and how the rate law for an...
To understand how elementary steps make up a mechanism and how the rate law for an elementary step can be determined. Very often, a reaction does not tell us the whole story. For instance, the reaction NO2(g)+CO(g)→NO(g)+CO2(g)NO2(g)+CO(g)→NO(g)+CO2(g) does not involve a collision between an NO2NO2 molecule and a COCO molecule. Based on experimental data at moderate temperatures, this reaction is thought to occur in the following two steps: NO2(g)+NO2(g)→NO3(g)+NO(g)NO2(g)+NO2(g)→NO3(g)+NO(g) NO3(g)+CO(g)→CO2(g)+NO2(g)NO3(g)+CO(g)→CO2(g)+NO2(g) Each individual step is called an elementary step. Together, these...
Experimental data is collected for the reaction shown below, with the following rate law: rate=k[NO2]2. What...
Experimental data is collected for the reaction shown below, with the following rate law: rate=k[NO2]2. What are the units of the rate constant for the reaction? NO2(g)+CO(g)→NO(g)+CO2(g) Trial123[NO2] (mol/L)0.060.060.09[CO] (mol/L)0.060.090.06Rate(mol L−1s−1)1.5408×10−61.5408×10−63.4668×10−6
You have the following reaction: NO2 (g) + CO (g) ⟶ NO (g) + CO2 (g)...
You have the following reaction: NO2 (g) + CO (g) ⟶ NO (g) + CO2 (g) The rate constant (k) at 701 K is 2.57 M-1s-1. If the activation energy is 150 kJ/mol, what is k at 895 K? R = 8.314 J/(mol*K) A) 680 M-1s-1 B) 443 M-1s-1 C) 2.58 M-1s-1 D) 0.950 M-1s-1 E) 6.52 M-1s-1
If the mechanism behind the reaction NO2(g) + CO(g) Ó NO(g) + CO2(g) is : 1- 2NO2(g) à 2NO(g) + O2(g) (slow) 2- NO(g) + CO(g) + O2(g) à NO2(g) + CO2(g) (fast) Then its rate law is: A) Rate = k [NO2] . [CO] B) Rate = k [NO2] . [CO2] C) Rate = k [NO 212 D) Rate = k [co]2
6. The rate law for the following reaction is rate=k[NO2] (F2]: 2NO2(g) + F2(g) → 2NO2F(g) The mechanism proposed for this reaction is as follows: (i) NO2(g) + F2(g) → NO2F(g) + F(g) (ii) NO2(g) + F(g) → NO2F(g) Which elementary step is the rate-determining step in this reaction? Explain your answer in 1-2 sentences.
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