1

answer

0

watching

61

views

13 Dec 2019

1. A first order reaction is seen to go from a reactant concentration of 0.0451 M to 0.0321 M in 41.8 seconds? How long (in seconds) after the reaction starts will the reactant concentration be 0.0180 M? I know the correct answer to this is 113 seconds, but I'm not sure how to get there.

2. HCOOH (g) â CO₂ (g) + H₂ (g)

At 555.0Â° C, the half life for this reaction is 23.5 min. How many seconds are needed for the initial concentration of HCOOH to decrease by a factor of 10? The correct answer to this is 4740 seconds, but again not sure how/why.

1

answer

0

watching

61

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

Casey DurganLv2

17 Dec 2019

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Related textbook solutions

Basic Chemistry

ISBN: 9780134138046

Principles of Chemistry Molecular Approach

ISBN: 9780134112831

Chemistry: Structure and Properties

ISBN: 9780134293936

Principles of Chemistry Molecular Approach

3rd Edition, 2014

ISBN: 9780321971944

Chemistry: A Molecular Approach

ISBN: 9780321809247

Chemistry: A Molecular Approach

ISBN: 9780134874371

Principles of Chemistry: A Molecular Approach

ISBN: 9780134895741

Chemistry: The Central Science

14th Edition, 2017

ISBN: 9780134414232

Related questions

Rate = -?[NOBr]/?t = k[NOBr]^2

2 NOBr(g) -> 2 NO(g) + Br2(g)

a) If the half-life for this reaction is 2.00 s when [NOBr]0 =0.900 M, calculate the value of k for this reaction.
I calculated this to be 0.556 L/mol*s

b) How much time (in seconds) is required for the concentration ofNOBr to decrease to 0.144 M?
This part is driving me crazy. I've done a ton of sample problemsand gone through the answers to similar questions on here, but Ikeep getting the wrong answer. Please help?

scarletsalmon597

Could you please answer these questions

1-

=======

2-

======

3-

======

4-

======

5-

======

6-

======

7-

=====

8-

======

9-

====

10-

======

11-

===

12-

=====

13-

The decomposition of N2O5 can be described by the equation Given these data for the reaction at 45degreeC in carbon tetrachloride solution, calculate the average rate of reaction for each successive time interval. Approximate the instantaneous rate of this reaction at time f = 40 s. The blue curve is the plot of the data. The orange line is tangent to the blue curve at t = 40 s. Consider the reaction described by the following equation. The rate law is What are the missing entries in the following table? What will the initial rate be if [A] is tripled and [B] is halved? Using the given data, determine the rate constant of this reaction. Using the given data, calculate the rate constant of this reaction. The rate constant for this first-order reaction is 0.620 s-1 at 400 degree C. How long (in seconds) would it take for the concentration of A to decrease from 0.770 M to 0.280 M? The rate constant for this zero-order reaction is 0.0120 M - s-1 at 300 degree C. How long (in seconds) would it take for the concentration of A to decrease from 0.800 M to 0.200 M? The rate constant for the reaction is 0.830 M 1 s-1 at 200 degree C. If the initial concentration of A is 0.00870 M, what will be the concentration after 795 s? For A products, time and concentration data were collected and plotted as shown here. Determine the reaction order, the rate constant, and the units of the rate constant. After 79.0 min, 40.0% of a compound has decomposed. What is the half-life of this reaction assuming first-order kinetics? A particular reactant decomposes with a half-life of 137 s when its initial concentration is 0.303 M. The same reactant decomposes with a half-life of 219 s when its initial concentration is 0.190 M. Determine the reaction order. What is the value and unit of the rate constant for this reaction? For each of the following cases, identify the order with respect to the reactant, A. The half-life of A decreases as the initial concentration of A decreases A threefold increase in the initial concentration of A leads to a ninefold increase in the initial rate. A threefold increase in the initial concentration of A leads to a 1.73-fold increase in the initial rate The time required for [A] to decrease from [A]0 to [A]o/2 is equal to the time required for [A] to decrease from [A]q/2 to [AJq/4.

Show transcribed image text The decomposition of N2O5 can be described by the equation Given these data for the reaction at 45degreeC in carbon tetrachloride solution, calculate the average rate of reaction for each successive time interval. Approximate the instantaneous rate of this reaction at time f = 40 s. The blue curve is the plot of the data. The orange line is tangent to the blue curve at t = 40 s. Consider the reaction described by the following equation. The rate law is What are the missing entries in the following table? What will the initial rate be if [A] is tripled and [B] is halved? Using the given data, determine the rate constant of this reaction. Using the given data, calculate the rate constant of this reaction. The rate constant for this first-order reaction is 0.620 s-1 at 400 degree C. How long (in seconds) would it take for the concentration of A to decrease from 0.770 M to 0.280 M? The rate constant for this zero-order reaction is 0.0120 M - s-1 at 300 degree C. How long (in seconds) would it take for the concentration of A to decrease from 0.800 M to 0.200 M? The rate constant for the reaction is 0.830 M 1 s-1 at 200 degree C. If the initial concentration of A is 0.00870 M, what will be the concentration after 795 s? For A products, time and concentration data were collected and plotted as shown here. Determine the reaction order, the rate constant, and the units of the rate constant. After 79.0 min, 40.0% of a compound has decomposed. What is the half-life of this reaction assuming first-order kinetics? A particular reactant decomposes with a half-life of 137 s when its initial concentration is 0.303 M. The same reactant decomposes with a half-life of 219 s when its initial concentration is 0.190 M. Determine the reaction order. What is the value and unit of the rate constant for this reaction? For each of the following cases, identify the order with respect to the reactant, A. The half-life of A decreases as the initial concentration of A decreases A threefold increase in the initial concentration of A leads to a ninefold increase in the initial rate. A threefold increase in the initial concentration of A leads to a 1.73-fold increase in the initial rate The time required for [A] to decrease from [A]0 to [A]o/2 is equal to the time required for [A] to decrease from [A]q/2 to [AJq/4.

Consider the reaction of carbon monoxide with oxygen to produce carbon dioxide.

2CO(g) + O2(g) -> 2 CO2(g)

At what temperature will this reaction be spontaneous according to Gibb's Energy?

DeltaH in kJ/mol for: CO(g) = -110.5, CO2(g) = -393.5
DeltaS in J/mol K for: CO(g) = 197.6, CO2(g) = 213.6, O2 = 205.0

This question was from my quiz and was a multiple choice question, the answer was "temps below 3273K" I'm not sure entirely if this question is asking for an estimate considering enough information might not be given, but an explanation of how you would go about doing it will be rewarded.

Weekly leaderboard

Homework Help 3,900,000

Chemistry 830,000

Start filling in the gaps now

New to OneClass?Sign up