The reaction of ammonium ion with nitrite ion in aqueous solution NH, + NO. →N₂ + 2H₂O is first order in NHA and first order in NO₂. 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 of the reaction was determined to be 3.72 x 105 M-s¹, when [NH,"]= 0.564 M and [NO₂] = 0.164 M. From this experiment, the rate constant is M¹.s

The reaction of ammonium ion with nitrite ion in aqueous solution NH, + NO. →N₂ + 2H₂O is first order in NHA and first order in NO₂. 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 of the reaction was determined to be 3.72 x 105 M-s¹, when [NH,"]= 0.564 M and [NO₂] = 0.164 M. From this experiment, the rate constant is M¹.s

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 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 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
Can you explain the concept? How to apply the concept to this problem and other problems?
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 =
The reaction of nitrogen dioxide with fluorine 2NO2+F2-->2NO2F is first order in NO2 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 or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n .
Please do it clearly...neat and clean !!!
What is the rate constant for the reaction?
Please don't provide handwritten solution ....
3. The time integrated rate law of a reaction involves a single reactant A of order (1/2) is:
Q2) Calculate the rate constant for the first order decomposition reaction of phosphine [PH3], M (at 120 °C): 4PH3(g)→ P4(g) + 6H₂(g)? .64 * 10 ^ - 2 Time (sec) a) 2.47 * 10 ^ - 2 * s ^ - 1 0 2.32 *10^ - 8 1.16 * 10 ^ - 2 (5.80 * 10 ^ - 3)/84 b) 28s ^ - 1 c) 4.64*10^ -2 overline s^ -1 56 d) 3.57 * 10 ^ - 2 * s ^ - 1
Q2
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.