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 NO2(g) + CO(g) CO2(g) + NO(g) has a rate constant of 2.57 M−1∙s−1 at...
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 rate constant at 701 K is measured as 2.57 M−1⋅s−1 and that at 895 K is measured as 567 M−1⋅s−1. Use the value of the activation energy (Ea=1.50×10^2kJ/mol) and the given rate constant of the reaction at either of the two temperatures to predict the rate constant at 476 K.
1.) If a random reaction A + B Products is first order with respect to A and second with respect to B, how is the rate impacted when the concentration of A and B are doubled? A) It increases by a factor of 2 B) It increases by a factor of 4 C) It increases by a factor of 8 D) It decreases by a factor of 4 E) Not enough information to determine 2.) You have the following reaction:...
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?
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 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.
A particular reaction has an enthalpy of 175.2 kJ and a reverse activation energy of 80.5 kJ. What is the activation energy for the forward reaction, that is, the reactants going to products? Report your answer in kilojoules to 4 sig figs, but do NOT include units. To test for blood circulation problems in a patient, a doctor injected a solution containing 8.9 ug of sodium-24 into their femoral artery. The circulation was then assessed by monitoring the radioactivity that...
A reaction has a rate constant of 0.0177 s-1 at 400.0 K. If the reaction has activation energy of 125 kJ/mol, calculate the rate constant at 500.0 K.A reaction has a rate constant of 0.0177 s-1 at 400.0 K. If the reaction has activation energy of 125 kJ/mol, calculate the rate constant at 500.0 K.
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