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
Hope it will help you.
Thankyou :)
The rate of the reaction: NO2(g) + CO(g) → NO(g) + CO2(g) was determined in three...
Reaction Equation: NO2 (g) + CO(g) ⟶ NO(g) + CO2 (g) Experiment Number Inital concentration of [NO2] (M) Inital concentration of [CO] (M) Initial rate (M/s) 1 0.200 0.200 5.00X10-4 2 0.200 0.800 8.00X10-3 3 0.600 0.200 5.00X10-4 A.) Determine the order (0, 1, or 2) with respect to NO2. B.) Determine the order (0, 1, or 2) with respect to CO.
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
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 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
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:
Consider the reaction: 2 NO(g) + O2 (g)--> 2 NO2 (g) The following data were obtained from three experiments using the method of initial rates: 3. Consider the reaction: 2 NO(g) + O2(g) → 2 NO2(g) The following data were obtained from three experiments using the method of initial rates: Initial [NO] Initial rate NO Initial [02] mol mol L-1 mol L-1 L-15-1 0.010 0.010 Experiment 1 Experiment 2 Experiment 3 0.020 0.010 2.5 x 10-5 1.0 x 10-4 5.0...
3. For the reaction C3H3(g) + 5 O2(g) ----> 3 CO2(g) + 4H20(1) the following rate data were determined at 30°C. Experiment Initial C3H8 Initial O2 id. Rate 0.200M 0.200 M 3.00 x 101 0.400 M 0.200 M 6.00 x 101 0.200 MO 0.400 M 1 .20 x 102 a) Determine the reaction order with respect to C3H8. b) Determine the reaction order with respect to 02. c) Calculate the rate constant at this temperature. d) Write the rate law...
4) A reaction is performed to study the reaction of nitrogen dioxide with carbon monoxide: NO2 + CO ---> NO + CO2 The following reaction rate data was obtained in four separate experiments. Experiment [NO2]0, M [CO]0, M Initial Rate, Ms-1 1 1.54 0.435 1.33 2 3.08 0.435 5.31 3 1.54 0.870 1.33 4 3.08 0.870 5.31 What is the rate law for the reaction and what is the numerical value of k? Complete the rate law in the box...