answer

watching

views

23 Nov 2019

Experiment 1:

Rate = k[BrO3-][Br-][H+]2

What would happen to the initial rate of reaction if thefollowing happpened?

a. Reactant A is a first order reactant, and [A] washalved?

b. Reactant B is a second order reactant, and [B] wastripled?

c. Reactant C is a zero order reactant, and[C]quadrupled?

d. Reactant D is a second order reactant, and [D]halved?

I'm stuck on how to apply the orders into the given rate toprovide what would happen in each instance above.

Thank you!!!

answer

watching

337

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Trinidad TremblayLv2

16 May 2019

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

1. For each of the following rate equations, describe what would happen to the rate if the concentration of reactant A was tripled and the concentration of reactant B is halved.

a. Rate = k[A][B]

b. Rate = k[A]2 [B]

c. Rate = k[A]2 [B]2

d. Rate = k[A][B]

2. If a reactant is used up according to a first order rate equation, and the initial concentration of the reactant is 3.2 mol L-1 , what is the concentration of the reactant after two half-lives have passed, and after six half-lives have passed?

amethystpug208

if a reactant is used up according to a first order rate law, and the initial concentration of the reactant is 3.2 mol L-1 , what is the concentration of the r reactant after two half-lives have passed and after six half-lives have passed?

Different Q, For each of the following rate laws, describe what would happen to the reaction rate if the concentration of reactant A was triple and the concentration of reactant B is halved. Rate=k[A] [B] Rate= k [A]2 [B] Rate=k [A]2 [B]2 rate= k [A] [B]3

goldotter472

The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line,y=mx+b.

Order	Integrated Rate Law	Graph	Slope
0	[A]=?kt+[A]0	[A] vs. t	?k
1	ln[A]=?kt+ln[A]0	ln[A] vs. t	?k
2	1[A]= kt+1[A]0	1[A] vs. t	k

Part A

The reactant concentration in a zero-order reaction was 5.00Ã10^?2M after 175 s and 4.00Ã10^?2M after 400 s . What is the rate constant for this reaction?

Part B

What was the initial reactant concentration for the reaction described in Part A?

Part C

The reactant concentration in a first-order reaction was 6.40Ã10^?2M after 50.0 s and 4.60Ã10^?3M after 60.0 s . What is the rate constant for this reaction?

Part D

The reactant concentration in a second-order reaction was 0.730 M after 210 s and 6.40Ã10^?2M after 705 s . What is the rate constant for this reaction?

Weekly leaderboard

Home

Homework Help 3,900,000

Chemistry 830,000

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related questions

Weekly leaderboard