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)
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
The activation energy for the reaction NO2(g)+CO(g)⟶NO(g)+CO2(g) is Ea = 200 kJ/mol and the change in enthalpy for the reaction is ΔH = -200 kJ/mol . What is the activation energy for the reverse reaction?
The activation energy for the reaction NO2(g)+CO(g)⟶NO(g)+CO2(g) is Ea = 150 kJ/mol and the change in enthalpy for the reaction is ΔH = -375 kJ/mol . What is the activation energy for the reverse reaction?
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 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
The reaction 2 NO2(g) → 2 NO (g) + O2(g) has rate constants of 2.70 x 10-2 M-1s-1 at 227 oC and 0.240 M-1s-1 at 277oC. What is the activation energy of this reaction? (Given: Arrhenius equation, k = Ae-Ea/RT ) A) 99.6 kJ/mol B) 22.8 kJ/mol C) 49.8 kJ/mol D) -22.8 kJ/mol E) 65.3 kJ/mol I'm unsure on how to do it since you're not given the frequency factor
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
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
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:
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