Practice ProblemATTEMPT
The reaction between
The experimental rate law is rate
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Chemistry
- The reaction A → products is first order. If the initial concentration of A is (6.0400x10^-1) M and, after (9.30x10^1) seconds have elapsed, the concentration of A has fallen to (2.710x10^-1) M, what is the rate constant of the reaction? Answer: ______x10 ____ units____arrow_forwardFor the reaction 2 NO(g) + O 2 (g) → 2 NO2 (g) have the following data. Experiment 1 2 3: [NO], M 0.010: 0.020: 0.010 [O 2 ], M 0.010 :0.010: 0.020 The speed of consumption of 2.5 x 10-5 1.0 x 10-4 5.0 x 10-5 NO, Ms -1 a) write the rate equation for the reaction b) calculate the rate constantarrow_forwardThe initial rate of the reaction 2 A + B → C + D was studied in a series of kinetics experiments. Trial Conc A (M) Conc B (M) Initial Rate (M/s) 1 0.300 0.100 0.000704 2 0.900 0.100 0.006334 3 0.900 0.300 0.006334 What is the experimental rate law for this reaction? Question 16 options: A) Rate = k[B]2 B) Rate = k[A]2 C) Rate = k[A] D) Rate = k[A]2[B] E) Rate = k[A][B]arrow_forward
- Part A Consider the reaction 2H3PO4→P2O5+3H2O2H3PO4→P2O5+3H2O Using the information in the following table, calculate the average rate of formation of P2O5P2O5 between 10.0 and 40.0 ss. Time (ss) 0 10.0 20.0 30.0 40.0 50.0 [P2O5][P2O5] (MM) 0 2.50×10−3 5.50×10−3 7.30×10−3 8.50×10−3 9.10×10−3arrow_forwardPRACTICE ANOTHER Identify the reaction intermediate or intermediates in the following multi-step mechanism. (Separate substances in a list with a comma.) Overall: 4 NO + 3 O2 + 2 H2O → 4 HNO3Step 1: 2 NO + O2 → 2 NO2Step 2: 4 NO2 + O2 + 2 H2O → 4 HNO3 ??????arrow_forwardThe reaction, A → products, is known to be second order with respect to the concentration of A and second order overall. The rate constant for the reaction is 0.0180 M-1·min-1 at a certain temperature.If the initial concentration of A is 0.580 M. What will be the concentration of A after 58.0 min?Answer MHow long would it take for 66.0% of the starting material (A) to undergo reaction?Answer minarrow_forward
- if a reaction is second order in B and the concentration of B increased from 0.0850M to 0.2975M, what should happen to the rate? experiment A B initial rate #1 0.20M 0.10M 3.50x10-3M/s #2 0.40M 0.10M 7.00x10-3M/s #3 0.40M 0.40M 7.00x10-3M/sarrow_forwardConsider the reaction to produce a block co-polymer below. A and B are different monomers. For example A could be limonene and B could be styrene. 2A + 3B → products If the rate law for the reaction is first order in A and second order in B, which of the following is the rate law for the reaction? Question 4 options: Rate = k[A][B] Rate = k[A]2[B]3 Rate = k[A][B]2 Rate = k[A]2[B] Rate = k[A]2[B]2arrow_forward. Consider the following reaction between mercury(II) chloride and oxalate ion: 2HgCl2(aq) + C2O42- ® 2Cl-(aq) + 2CO2(g) + Hg2Cl2(s) The initial rate of this reaction was determined for several concentrations of HgCl2 and C2O42-, and the following rate data were obtained: Experiment [HgCl2] (M) [C2O42-] (M) Rate (M/s) 1 0.105 0.15 1.8 x 10-5 2 0.105 0.30 7.1 x 10-5 3 0.052 0.30 3.5 x 10-5 4 0.052 0.15 8.9 x 10-6 a) What is the rate law for this reaction? b) What is the value of the rate constant? c) What is the reaction rate when the concentration of HgCl2 is 0.080 M and that of C2O42- is 0.10 M if the temperature is the same as in the above experiments?arrow_forward
- Select the rate law that corresponds to the data shown for the following reaction: 2 A + 3 B → 2C Initial [A] 0.15 M 0.15 M 0.45 M Initial [B] 0.12 M 0.24 M 0.24 M Initial Rate 0.10 M/s 0.20 M/s 1.80 M/s (One of the options below is correct) a. rate = k[A]3[B] b. rate = k[A]3[B]2 c. rate = k[A]3 d. rate = k[A]2[B] e. rate = k[A]2[B]3arrow_forwardThe reaction, A → products, is known to be zeroth order with respect to the concentration of A and zeroth order overall. The rate constant for the reaction is 0.1400 M·hr-1 at a certain temperature.If the initial concentration of A is 0.750 M. What will be the concentration of A after 3.8 hr?Answer MHow long would it take for 95.0% of the starting material (A) to undergo reaction?Answer hrarrow_forwardWhich of the following is the Rate Law for this reaction? You do not need to solve for k in this problem. Br2 + 2 NO2 → 2 NO2Br Experiment [Br2] (M) [NO2] (M) Initial Rate (M/s) 1 0.100 0.100 0.103 2 0.100 0.200 0.205 3 0.200 0.200 0.819 Rate = k [Br2]2[NO2]2 Rate = k [Br2]2[NO2] Rate = k [Br2] [NO2] Rate = k [Br2][NO2]2 Rate = k [NO2Br]2arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning