A reaction is performed to study the reaction of nitrogen dioxide with fluorine: 2 NO₂+ F22 NO₂F The following reaction rate data was obtained in four separate experiments. Experiment 1 2 3 Rate = [NO₂]0, M 0.690 1.38 0.690 1.38 k= [F₂]0, M 2.40 2.40 4.80 4.80 M-¹5-1 Initial Rate, Ms-1 What is the rate law for the reaction and what is the numerical value of k? Complete the rate law in the box below. Remember that an exponent of '1' is not shown and concentrations taken to the zero power do not appear. 1.85x10-4 3.71x10-4 3.71x10-4 7.42x10-4

Consider the gaseous reaction of mononitrogen monooxide with molecular hydrogen to produce molecular nitrogen and water. What is the reaction rate between t = 10 s and t = 30 s?         Time (s)       [H2]           0      1.00         10    0.805         20    0.663         30    0.491          40    0.376          50    0.308     -0.0127 M/s     0.00785 M/s     0.0255 M/s     0.0157 M/s     -0.0157 M/s

The balanced equation for a given reaction is 4 X + 3 Y → P. The following data regarding initial reaction rates were collected in the lab. What is the rate law for the reaction? Trial [X] (M) [Y] (M) Rate (M/s) 1 0.020 0.060 3.40 x 10–3 2 0.020 0.120 2.72 x 10–2 3 0.080 0.060 1.36 x 10–2

Consider the following general reaction for which gases A and B are mixed in a constant volume container: A(g) + B(g) -> C(g) + D(g) Match what happens to the rate of the reaction under the following changes: (consider each change separately) v all of gas B is removed from the container more gas A is added to the container the temperature of the container is increased there is no change to the reaction rate ya catalyst is added to the container I. the reaction proceeds at a faster rate v gas D is also added to the container the reaction proceeds at a slower rate II. some of gas B is removed from the container Iy the reaction does not proceed at all the volume of the container is increased

Determine the rate law and calculate the rate constant for this reaction: 2 NO (g) + Br₂(1)→2 NOBr (g) Initial [Br₂]/M Expt. 1 2 3 Initial [NO]/M 0.10 0.20 0.20 0.10 0.10 0.30 Initial rate/M.s-¹ 1.30 x 10-³ 5.20 x 10-³ 1.56 x 10-²

Consider the reaction: NO2 + 03 → NO3 + 02 [NO,], M [03], M Rate, M/s 6.30 x 10-3 Experiment 1 0.21 0.70 1.89 x 10-2 3.15 x 10-3 0.63 0.65 3 0.21 0.35 4 0.42 0.35 6.30 x 10-3 Calculate the rate of [NO3] production at 0.84 M [NO2]and 1.4 M [03]. Final answer must be rounded off to 2 decimal places, and shall NOT have any units.

What is the rate of the reaction when A=0.43M and B=0.31M?

g.

A mechanism for a fake overall chemical reaction is shown below:   Step #1:  X3 (g)  +  QX (g)  →  QX2 (g)  +  X2 (g)   Step #2:  QX2 (g)  +  X (g)  →  QX (g)  +  X2 (g) Which species would be defined as a catalyst? X QX2 X3 X2 QX