5. The following data were obtained for the gas-phase decomposition of nitrogen dioxide at 300 °C, NO2 ) NO(g) + 02(g): INO2 (M) Time (s) 0.01000 0.0 50.0 0.00787 0.00649 100.0 200.0 0.00481 300.0 0.00380 Is the reaction first or second order in NO2? What is a value of rate constant of this reaction?

A decomposition reaction follows second order kinetics with a rate constant, k = 0.0137 M-1 min-1. If the initial concentration of the reactant is 0.866 M, what is the concentration after 5 minutes? Report your answer to the thousandths place and do not include units.

The decomposition of nitrous oxide at 565 °C N20(g)N2(g) + ½ O2(g) is second order in N20. In one experiment, when the initial concentration of N20 was 1.85 M, the concentration of N20 dropped to 0.501 M after 927 seconds had passed. Based on these data, the rate constant for the reaction is

The decomposition of aqueous hydrogen peroxide (H2O2) to gaseous oxygen and water is a 1st order process.  If it takes 6.0 h for the concentration of H2O2 to decrease from 0.40 M to 0.20 M, how many hours are required for the concentration to decrease from 0.70 M to 0.35 M?

Data for the decomposition of nitrosyl bromide: 2NOBrg) → 2NO(9) + Brz) is given below: ---- Time (s) [NOBI] (mol/L) Calculate the average rate of decomposition of nitrosyl bromide during the time interval 2.0 0.0071 4.0 0.0055 6.0 0.0045 8.0 0.0038 10.0 0.0033 0.0100 (a) 0 to 10 seconds (b) 2.0 to 4.0 seconds Plot the data then determine the specific rate at 7 seconds by drawing a line tangent to the curve.

The gas phase decomposition of hydrogen iodide at 700 K HI(g)- → H₂(g) + ½ l₂(g) is second order in HI with a rate constant of 1.20×10-³ M-¹s-¹. How much time is required for the concentration of HI to drop to 0.418 M if its initial concentration is 2.50 M? S

The decomposition of N2O5 to NO2 and O2 is first order with respect to the reactant N₂05 and first order overall. The rate constant for the reaction at 70.°C is 6.82x10-3 s-1. The reaction is started with 0.300 mol of N205 in a 0.500L container. What will the concentration of N2O5 be after 1.50 minutes? O a. 0.594M O b. 0.438M O c. 0.297M O d. 0.325M O e. 0.162M O f. 0.253M

The rate constant for this zero-order reaction is 0.0240 M •s= at 300 °C. A products > How long (in seconds) would it take for the concentration of A to decrease from 0.890 M to 0.270 M? t = S

The half-life for the second-order decomposition of H₂S is 6.3 seconds when the initial concentration of HI is 0.027 M. What is the rate constant for this reaction?

A reaction is found to be first-order with a rate constant of 0.0525 s–1. If the reaction initially began with 5.25 M reactant, how long (in s to the nearest whole number) will it take for 0.20 M reactant to be consumed?