The reaction 2NOB →2NO +Br2 exhibits the rate law A[NOBr]? A[NOBI] At Rate = where k= 1.0 x 10-5 Ms- at 25°C. This reaction is run where the initial concentration of NOBR !! ([NOBIJ0) is 0.30 M. What is one half-life for this experiment? O 3.0 s O 1.5 x 10-5 s O 6.9 x 104s O 3.3 x 10 s none of these

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

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

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

Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.0317 M¹-s¯¹) [₂0₂] S Suppose a vessel contains N₂O5 at a concentration of 0.440 M. Calculate the concentration of N₂O5 in the vessel 480. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 ? X S

Consider the initial-rate data at a certain temperature in the table for the reaction described by 2 NO₂(g) + O₂(g) → N₂O5 (g) + O₂(g) Determine the value and units of the rate constant, k. k = X10 TOOLS [NO2], (M) [03]o (M) 0.650 0.800 1.10 0.800 1.76 1.40 Units: Initial rate (M/s) 3.12 x 104 5.28 x 104 14.78 x 104

3. An experiment was carried out to determine the rate law for the following reaction: 19152 2NO( )+0( ) → 2NO( ) Where the rate law is: par Rate = k[NO] [0] The experiment was repeated three times and the following data recorded: Experiment # Initial [NO] (M) Initial [0] (M) Rate (M/s) 1 ullo2 M0.015 0.015 2 0.030 0.015 3 0.015 0.030 of in Determine the value of x in the rate law (order of reaction with respect to NO) by comparing experiments 1 and 2 in Equation 13 reaction with respect to O₂) by comparing experiments 1 and 3 in equation 13. 0.048 0.192 0.096

General Chemistry 4th Edition McQuarrie • Rock • Gallogly dUniversity Science Books presented by Macmillan Learning The reaction C,H¿ (g) → 2 C,H¿(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 × 10-8 s-!. What is the value of the rate constant at 840.0 K? k =

Consider the reaction below at 100oC  T2U (g)  ⟶⟶ 2 T (g)  + U (g)  When [T2U] = 0.250 M, the reaction rate is 9.30 x 10-3 M/s, and when [T2U]o = 0.144 M, the reaction rate is 3.09 x 10-3 M/s, A. Which is the rate law of this reaction? B.  which is the numerical value of the specific-rate constant, k, for this reaction?  C. Which are the units for the specific rate constant, K? D. At whic rate is T generaten when [T2U] is 0. 111 M? E. if given an initial reactant concentration [T2U]o = 0.250 M, what is [T] after 15 minutes have elapsed?

Consider this reaction: 2H,PO, (ag) – P,0, (aq)+ 3H,0 (aq) At a certain temperature it obeys this rate law. rate = (0.392 M-1.s Suppose a vessel contains H, PO, at a concentration of 0.520 M. Calculate how long it takes for the concentration of H, PO, to decrease to 12.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.