The decomposition of ammonia on a platinum surface at 856 °C follows the chemical equation:\[ \text{NH}_3 \rightarrow \frac{1}{2} \text{N}_2 + \frac{3}{2} \text{H}_2 \]This reaction is zero order in \(\text{NH}_3\) with a rate constant of \(1.50 \times 10^{-6} \, \text{M} \, \text{s}^{-1}\).If the initial concentration of \(\text{NH}_3\) is \(1.18 \times 10^{-2} \, \text{M}\), the concentration of \(\text{NH}_3\) will be \(3.45 \times 10^{-3} \, \text{M}\) after a certain number of seconds have passed.---**Instructions:**- Use the references to access important values if needed.- Calculate the time it takes for the concentration to decrease from the initial value to the given concentration.**Interactive Components:**- Submit Answer- Retry Entire Group- Remaining Attempts: 9Options for navigation are present at the bottom:- Email Instructor- Save and ExitThis is displayed on a user interface provided by Cengage Learning, with options for technical support.

Given, initial concentration of NH3, [Ao] = 1.18 x 10-2 M concentration of NH3 at time t…

The decomposition of ammonia on a platinum surface at 856 °C NH3 →1/2 N2 + 3/2 H2 is zero order in NH3 with a rate constant of 1.50×10-6 M s-1. If the initial concentration of NH3 is 1.18×10 M, the concentration of NH3 will be 3.45×103M after seconds have passed. Submit Answer Retry Entire Group 9 more group attempts remaining

The decomposition of ammonia on a platinum surface at 856 °C NH3 →1/2 N2 + 3/2 H2 is zero order in NH3 with a rate constant of 1.50×10-6 M s-1. If the initial concentration of NH3 is 1.18×10 M, the concentration of NH3 will be 3.45×103M after seconds have passed. Submit Answer Retry Entire Group 9 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

Answer all parts
Want solution asap....
< 2:19 A) S-¹ B) M S-¹ What are the units for the rate constant of a first-order reaction? C) M-¹ s¹ D) M-² S-¹ Question 11 of 15 E) s M-¹ 5GW Tap here or pull up for additional resources Submit
Part B Consider the second-order reaction: 2HI(g)→H₂(g) + I₂(g) Use the simulation to find the initial concentration [HI], and the rate constant k for the reaction. What will be the concentration of HI after t = 5.44x10¹0 s ([HI]) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures. ► View Available Hint(s) for Part B for Part do for Part redo for Part B res@or Part B keyboard shortcuts for Part B help for Part B [HI] = 1.6810³ Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining mol L
Need help
I don’t know how to find the activation energy in this problem
ASAP please
Chemistry
Need help pls
empt 1 2 CIO2 (aq) + 2 OH (aq)- CIO3 (aq) + CIO2 (aq) H2O 2: Initial Rate (M/s) 0.0248 0.00276 0.00828 Trial [CIO21 0.060 0.020 0.020 0.030 0.030 0.090 What is the order of the reaction with respect to CIO2? 1 23
Part A Which of the following represents the integrated rate law for a first-order reaction? Ea O In는 = ()+ InA k1 k2 R O [A]t – [A]o = -kt | O k= Ae(Ea/RT) O In [A]. ) = -kt [A]o 1 kt [A]. %3D Submit Request Answer
[A] (M) 1/IA] In [A] (s) 0.00 0.500 -0.693 2.00 20.0 0.389 0.944 2.57 40.0 0.303 1.19 3.30 60.0 0.236 1.44 4.24 80.0 0 184 1.69 5.43 Part A What is the order of this reaction? > View Available Hint(s) What is the activation energy of this reaction? Express your answer to three significant figures and include the appropriate units.