Hydrogen gas reduces NO to N2 in the following reaction:$$2H2​(g)+2NO(g)2H2​O(g)+N2​(g)The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C with the following results: Experiment [H2]0 (M) [NO]0 (M) Initial Rate (M/s) 1 0.212 0.136 0.0387  2 0.212 0.272 0.0777  3 0.424 0.544 0.615  4 0.848 0.544 2.47      Determine the rate constant for the reaction at 1500°C.     M-xs-1

2. Consider the reaction A+2B C whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: [v] (M) (M) (M/s) [B] Rate Trial 1 0.10 0.050 6.0x10-4 0.10 0.100 1.2x10-3 3 0.20 0.050 2.4x10-3 Part B Provide

1. At elevated temperatures, nitrous oxide decomposes according to the equation2N2O(g)⟶2N2(g)+O2(g) Time (min) 0 60 90 300 600 [N2O] 0.250 0.228 0.216 0.128 0.0630 Given the following data, determine whether the reaction is zeroth, first, or second order. a) first b) second c) zeroth

Consider the following complex reaction: A + 2B → C whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [A](M) [B](M) Rate(M/s) 1 0.400 0.050 9.60 × 10−3 2 0.400 0.100 1.92 × 10−2 3 0.800 0.050 3.84 × 10−2 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law. Express your answer to three significant figures. Include units for k.

For the question above, calculate the value of k (include units). Show your work.

Consider the following complex reaction:   2NO2(g) + O3(g) →  N2O5(g) + O2(g) whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [NO2](M) [O3] (M) Rate (M/s) 1 0.20 0.40 0.25 2 0.40 0.40 0.50 3 0.40 1.20 1.50    What is the rate law for this reaction? Write the value for k to two significant figures in the first box. Select the units for k and concentration terms in the second box.