A) the rate of a reaction is dependent on the equilibrium constant. B) the rate of a first order reaction changes as the reactant is used up. C) second order reactions are always faster than first order reactions. D) if the rate of a reaction doubles when the concentration of a reactant doubles, the reaction is second order with respect to that reactant.

A) the rate of a reaction is dependent on the equilibrium constant. B) the rate of a first order reaction changes as the reactant is used up. C) second order reactions are always faster than first order reactions. D) if the rate of a reaction doubles when the concentration of a reactant doubles, the reaction is second order with respect to that reactant.

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

Which of the following statements is FALSE about molecularity of kinetic reactions? a) Multimolecular reactions rarely occurs in enzyme kinetics. b) Unimolecular reactions are defined as First-order reactions. c) Bimolecular reaction rates double when the reactant concentration doubles. d) The half-life of the bimolecular reaction depends on the concentration of the reactant. e) When the amount of one of two starting reactants is very low, it becomes the rate limiting reactant.
The first-order rate constant for the decomposition of a certain drug is 0.215 /month a) if 10.0 g of the drug is stored for one year, how many grams of the drug will remain at the end of the year? b) what is the half-life of the drug? c) How long will it take to decompose 65% of the drug?
How do you solve this?
Given the following proposed mechanism, predict the rate law for the overall reaction. 2NO₂+ Cl₂ → 2NO₂CI (overall reaction) Mechanism NO₂+ Cl2 → NO₂CI+ Cl NO 2 + Cl → NO₂CI A) Rate = k[NO₂] [Cl₂] C) Rate = k[NO₂][CI] = slow fast B) Rate = k[NO₂]²[C]² D) Rate = k[NO₂CI][CI]² E) Rate= k[NO₂CI]
If a reactant is 1st order and the concentration is doubled, how fast is the rate?
Can someone please help with question 3
Experimentally one finds that if the concentration of (CH3)3CBr is doubled, the rate of the reaction doubles. One also finds that if the concentration of CH3CH2OH is doubled, the rate of the reaction quadruples. Which of the following correctly describes the kinetic of this reaction? A) The reaction is third order overall B) The reaction is first order in CH3CH2OH C) The reaction is second order overall D)The reaction is first order overall E) none of the above
Give the characteristic of a first order reaction having only one reactant. The rate of the reaction is not proportional to the concentration of the reactant. The rate of the reaction is proportional to the square of the concentration of the reactant. The rate of the reaction is proportional to the square root of the concentration of the reactant. The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. The rate of the reaction is directly proportional to the concentration of the reactant.