For the reaction 3AE) + 2B(g) - 2C(g) + 2D(g) the following data were collected at constant temperature. Determine the correct rate law for this reaction. Trial Initial [A] Initial [B] Initial Rate (mol/L) (mol/L) (mol/(L-min)) 1 0.200 0.100 2.80 x 10 2 2. 0.100 0.100 3.5 x 103 3. 0.200 0.200 1.12 x 101 0.300 0.200 3.78x 10-1 OA Rate= k[A][B]² O B. Rate = k[A]PB] OC Rate = k[A] [B] O D. Rate = k[A]B] OE Rate = k[A]°B] QUESTION 17 Which of the following is a reaction intermnediate?

Consider the reaction 2N2O5(g) → 4NO2(g) + O2(g). Use the time-monitored concentration data to verify that the reaction is first order. Supply the regression statistics obtained by trying several integrated rate laws. Time, s [N2O5], M 0.0 0.100 30.0 0.090 60.0 0.080 90.0 0.070 120.0 0.060 Coefficients of determination (supply r2 up to four decimal places). zero order:  first order:  second order:

Consider this reaction: 2N,03 (g) → 2N,04(g) +O2 (g) At a certain temperature it obeys this rate law. rate =(167. Ms")[N,0, Suppose a vessel contains N,O, at a concentration of 0.220M. Calculate the concentration of N,0, in the vessel 0.200 seconds later. You may assume no 12 other reaction is important. Round your answer to 2 significant digits. () M x10

25. The reaction 2 NO2(g) + O3(g)  N2O5(g) + O2(g) was studied at a certain temperature with the following results:   Experiment [NO2(g)] (M) [O3(g)] (M) Rate (M/s)   1 0.502 0.502 21600 2 0.502 1.00 43100 3 1.00 0.502 43100 4 1.00 1.00 85800 (a) What is the rate law for this reaction? Rate = k [NO2(g)] [O3(g)] Rate = k [NO2(g)]2 [O3(g)]   Rate = k [NO2(g)] [O3(g)]2 Rate = k [NO2(g)]2 [O3(g)]2 Rate = k [NO2(g)] [O3(g)]3 Rate = k [NO2(g)]4 [O3(g)] (b) What is the value of the rate constant?(c) What is the reaction rate when the concentration of NO2(g) is 0.505 M and that of O3(g) is 1.37 M if the temperature is the same as that used to obtain the data shown above?______ M/s

5. The following initial rate data were obtained for the reaction a. C. 2C1O₂(aq) + 2OH(aq) → CIO3(aq) + ClO₂ + H₂O [CIO₂] 0.024 0.018 0.024 Write the rate law for this reaction. [OH-] 0.011 0.011 0.014 b. Calculate the rate constant and specify units. Initial Rate (Mos¹) 7.27 x 10-4 4.09 x 10-4 9.25 x 10-4 Calculate the rate when the [CIO₂] = 0.75 M and [OH-] = 0.0250 M.

x10 The rate law for the reaction NH(aq) + NO,lag) - N₂ (g) + 2 H₂O (1) is given by rate = k[NH][NO2]. At At a certain temperature, the rate constant is 4.40 × 10-4 1 M.s Calculate the rate of the reaction at that temperature if [NH] = 0.261 M and | [NO]=0 = 0.210 M. Be sure your answer has the correct number of significant digits. G 口・

Give typed full explanation not a single word hand written otherwise leave it

Consider the reaction 2HI→ H₂+I2. The rate of disappearance of HI follows the second order rate law. A[HI] = -k[HI]² At The rate constant kis 2.01 x 10-2 M-1s-1. What was the initial concentration of HI (in units of molarity) if the concentration of HI was found to be 0.262 M after t = 45.0 s? Report your answer using three significant figures. Provide your answer below: M rate

1) Write a basic form of the rate law for the following reaction. ClO4 + 8Br + 8H* → Cl + 4B12 + 4H2O Rate

Consider this reaction: 2NH3 (g) → N, (g)+3H, (g) At a certain temperature it obeys this rate law. rate = (0.0324 Ms)[NH,] -1 Suppose a vessel contains NH, at a concentration of 1.37M. Calculate how long it takes for the concentration of NH, to decrease to 0.233 M. You may assume no other reaction is important. Round your answer to 2 significant digits. S x10