**Educational Transcript on Zero-Order Kinetics Problem:**A certain chemical decomposes with zero-order kinetics. If the rate constant, \( k \), is \( (5.86 \times 10^{-5}) \, \text{M s}^{-1} \) and the initial concentration of the chemical is \( 0.700 \, \text{M} \), how many seconds would it take for the molarity to be \( (5.7300 \times 10^{-3}) \, \text{M} \)?**Instructions for Answering:**- Enter your answer in scientific notation with 3 significant figures.- Do not include any units in your answer.- Do not round any intermediate calculations.**Note:** Your answer is assumed to be reduced to the highest power possible. A first-order reaction has a half-life of (6.34×10^1) minutes. How many minutes would it take for the only reactant to decrease to 12.5% of its initial concentration?Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer.Do not round any intermediate calculations.Note: Your answer is assumed to be reduced to the highest power possible.

Since you have asked multiple questions, we will solve the first question for you. If you want any specific question to be solved then please specify the question number or post only that question.

Science

Chemistry

A certain chemical decomposes with zero-order kinetics. If the rate constant, k, is (5.86x10^-5) M s1 and the initial concentration of the chemical is 0.700 M, how many seconds would it take for the molarity to be (5.7300x10^-3) M?

A certain chemical decomposes with zero-order kinetics. If the rate constant, k, is (5.86x10^-5) M s1 and the initial concentration of the chemical is 0.700 M, how many seconds would it take for the molarity to be (5.7300x10^-3) M?

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

For the reaction AB(g) —>A(g) + B(g) the rate law is determined to be rate =k[AB]^2 and k=0.255 L/mol-min. If the initial concentration of AB is 1.00M, how long will it take for the concentration of AB to fall to 0.40M?
The decomposition of AB(g) is second order in AB. AB(g) --> A(g) + B(g) At a certain temperature, the rate constant is k=0.20 L/mol-s. If you begin a reaction with 1.00 M AB, how long will it take for the concentration of AB to drop to 0.50 M? Write your answer with 2 significant figures in units of seconds.
Hydrogen iodide decomposes at 800 K via a second-order process to produce hydrogen and iodine according to the following chemical equation. 2 HI(g) → H2(g) + I2(g) At 800 K it takes 142 seconds for the initial concentration of HI to decrease from 6.75 × 10-2 M to 3.50 × 10-2 M. What is the rate constant for the reaction at this temperature?
Consider the following rate law for the reaction A + B → products. rate = k{A}2{B}2 The reaction is order with respect to A, order with respect to B, and order overall.
The reaction so2cl2(g)→so2(g)+cl2(g) is first order. At 660 k it has a rate contsant of 4.5 X 10^-2 s^-1 Determine the concentration of SO2Cl2 at 15.2 seconds, if the initial concentration is 0.583 M.
Consider the reaction 2AB(g) → A2(g) + B2(g). If [AB] at 96 minutes was 0.71OM and dropped to 0.520M by 320.minutes, calculate the rate of consumption during this time frame.
The decomposition of ethylene oxide (CH₂)₂O(g) → CH₄(g) + CO(g) is a first order reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 613 K.
NOBr(g) decomposes to form NO and Br2 by the reaction 2 NOBr(g) + 2 NO(g) + Br2(8) It is found that the reaction is second order in NOBr. The rate constant has been found to be 0.170 M-1 s1. In a situation where the initial concentration of NOBr in a vessel is 0.690 M, how long will it take for the concentration of Br2 to reach 0.180 M? (Assume, of course, that there was no Br in the vessel to begin with.) Report your result in seconds with one decimal place but do not put units in the
The decomposition of ethylene oxide (CH₂)2O(g) → CH4(g) + CO(g) is a first order reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 631 K.
For Rate = k[A]4[B]3, determine the order with respect to reactants and determine the overall reaction order. Express your answer numerically. Order with respect to A = Order with respect to B = Overall order =
Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0086 M's : 2 N,0 (g) → 2 N2 (g) + 0, (g) Suppose a 300. mL flask is charged under these conditions with 100. mmol of dinitrogen monoxide. How much is left 10. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. x10 미