The gas phase reaction of hydrogen with iodine H₂+ 12 → 2HI is first order in H₂ and first order in I2. Complete the rate law for this reaction in the box below. Use the form [A] [B]", where '1' is understood for m, n... (don't enter 1) and concentrations taken to the zero power do not appear. Rate In an experiment to determine the rate law, the rate constant was determined to be 2.39 x 10-18 M's. Using this value for the rate constant, the rate of the reaction when [H2]=0.0636 M and [12]=0.0154 M would be M/s. Submit Answer Retry Entire Group more group attempts remaining

The gas phase reaction of hydrogen with iodine H₂+ 12 → 2HI is first order in H₂ and first order in I2. Complete the rate law for this reaction in the box below. Use the form [A] [B]", where '1' is understood for m, n... (don't enter 1) and concentrations taken to the zero power do not appear. Rate In an experiment to determine the rate law, the rate constant was determined to be 2.39 x 10-18 M's. Using this value for the rate constant, the rate of the reaction when [H2]=0.0636 M and [12]=0.0154 M would be M/s. Submit Answer Retry Entire Group more group attempts remaining

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The reaction of nitrogen monoxide with ozone at 25 °C NO + O3 NO2 + 02 is first order in NO and first order in 02. Complete the rate law for this reaction in the box below. Use the form k[A]"[B]"... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 111 M-ls1. Using this value for the rate constant, the rate of the reaction when [NO] = 0.117 M and [O3] = Ms 4.59x10-2 M would be
Please don't provide handwritten solution....
The red are the different options…just the LAST 2 please. Activation energy and frequency factor
4. Of course, this proposed law is hypothetical. Using the following data collected experimentally (probably using a UV/vis spectrometer ©), determine the rate law for this reaction. Include reaction order and the value and units for k. Please show your work, including any graphs you make. Time (s) [NO2], M 1.00х10-2 60 6.83x10-3 120 5.18x10-3 180 4.18x10-3 240 3.50х10-3 300 3.01х10-3
The gas phase reaction of hydrogen with iodine H₂+I2 → 2HI is first order in H₂ and first order in I2. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 2.03 x 10-18 M¹s¹. Using this value for the rate constant, the rate of the reaction when [H₂] = 0.0356 M and [1₂] = 0.0123 M would be M/s.
The graph below depicts the consumption of reactant A during a first-order reaction. (Enter all values to two significant figures.) [A], (M) 0.3 0.25 0.2 0.15 0.1 0.05 5 10 15 20 25 30 35 40 45 50 55 60 65 Using the graph, determine the half-life of the reaction. S (b) Calculate the rate constant and its units. ??? Time (s) Submit Answer
The reaction of nitrogen dioxide with fluorine 2 NO2 + F2 → 2 NO2F is first order in NO, and second order overall. Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate =
It is known that a reaction that takes place in a single step and proceeds as written below is 1st degree; xA + yB ...........> C What is the molecular value, rate equation and half-life of the reaction?
Q2
The reaction of UO,* with hydrogen ion in aqueous solution 2 UO,* + 4 H* → U** + UO2²* +2 H2O is second order in UO,* and third order overall. Complete the rate law for this reaction in the box below. Use the form k[A]™[B]"... , where 'l' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate =
The rearrangement of cyclopropane to propene at 500 °C(CH2)3CH3CH=CH2is first order in (CH2)3. During one experiment it was found that when the initial concentration of (CH2)3 was 0.170 M, the concentration of (CH2)3 dropped to 0.0491 M after 1304.0 s had passed.Based on this experiment, the rate constant for the reaction is ______s-1.
At a certain temperature this reaction follows second-order kinetics with a rate constant of 1.7M 2N₂O, (g) → 2N₂O₂(g) + O₂(g) Suppose a vessel contains N₂O, at a concentration of 1.18M. Calculate how long it takes for the concentration of N₂O, to decrease to 7.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. TEET olo F