Time and concentration data were collected for the reaction0.520.48A→ products0.44t (s)[A] (M)0.40 -0.52200.432 0.36400.350.32 -600.290.28800.230.241000.190.20The blue curve is the plot of the data. The straight orange lineis tangent to the blue curve at t = 40 s.0.160 10 20 30 40 50 60 70 80 90t (s)Approximate the instantaneous rate of this reaction at timet = 40 s.instantaneous rate:M/s[A] (M)

Answered: Image /qna-images/answer/ec1d41a3-ded9-4e7d-ba2d-ea3c24066a23.jpg

Answered: Approximate the instantaneous rate of…

Science

Chemistry

Approximate the instantaneous rate of this reaction at time t = 40 s.

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter13: Kinetic Methods

Section: Chapter Questions

Problem 9P

See similar textbooks

Related questions

Q: What is the reaction rate constant given the plot of the reaction of reactant A with respect to time…

A: here we are required to find the rate constant for the first order reaction

Q: Given the first order reaction: Y Z It is found that this reaction is 40.0% complete at the end of…

A: Given :- Y → Z (first order reaction) t = 40 min Completion of reaction = 40% To…

Q: A certain first-order reaction A ->B is 25% complete in 42 min at 25°C. What is the half-life of the…

Q: Calculate the initial concentration for a first order reaction with a final concentration of 0.403…

A: GivenOrder of reaction = 1Final concentration = 0.403 Mk = 0.00721 min-1t = 43.2 minInitial…

Q: The half life of a first order reaction is 28 second.what is its rate constant?

A: Half life (t1/2) :- " The time required for half of the reactants to convert into products is called…

Q: If the initial concentration of a reactant participating in a first- order reaction is increased…

A: The reaction rate or rate of reaction is the speed at which a chemical reaction takes place, defined…

Q: A certain first-order reaction has a rate constant of 0.00950 1/min at 300 K. What is the half-life…

A: Half life is the time when the concentration of reactants becomes half.

Q: Based on the data provided, what is the rate constant (with units) for this reaction? Trial Initial…

Q: how much time is required for 50% of the initial quantity of reactant to be consumed?

Q: What is the instantaneous rate of the reaction at t = 800. s?

A: Rate of reaction is the rate at which products are formed or reactants react. Instantaneous rate of…

Q: After 55.0 min, 11.0% of a compound has decomposed. What is the half‑life of this reaction assuming…

Q: A second order reaction is carried out in 25% after 60 minutes, if the initial concentration of the…

Q: A certain first-order reaction is 31.5 percent complete in 4.50 min at 25°C. What is its rate…

A: Rate of reaction represents the change of concentration of a reactant or a product with respect to…

Q: The rate constant for a first order reaction is 0.0640 1/s. What is the half-life for this reaction?

Q: A second order reaction with respect to Reactant A has an initial concentration of 0.15 M A, and a…

A: Given that : The concentration of Reactant A = 0.15 M Rate constant = 1.38 x 10-3 L/mol.s It is…

Q: The reaction rate constant for the first order reaction is 1.15x10-3s-1. Determine the half-life of…

Q: What fraction of a reactant has been consumed after 4 half-lives in a first-order reaction?

A: The rate of the reaction is referred to as the change in the molar concentration in a distinct…

Q: A certain first-order reaction has a rate constant of 0.00710 1/min at 300 K. What is the half-life…

A: The relationship between rate constant and half life for first order reaction is - Half life,…

Q: Calculate the final concentration for a second order reaction with a initial concentration of 0.643…

A: Second-order reaction means the rate is directly proportional to the square of the reactant…

Q: Calculate the activation energy of a first-order reaction that is 20% completein 15 minutes at 40 °C…

A: It is given that a first order reaction is 20% complete at 15 minutes at 40°C and 20% complete at 3…

Q: A second-order reaction has a half-life of 10 s when the initial concentration of reactant is 0.99…

Q: 1st order reaction is 27.0% complete at the end of 208 seconds. What is the value of rate constant…

Q: Hydrolysis of a hormone is a first-order reaction with a rate constant of 0.125 years-1. What will…

A: Use first order kinetic formula to get all the answer.

Q: The rate constant for this first‑order reaction is 0.0130 s−1 at 400 ∘C. A⟶products After how…

Q: Chemical B reacts by first-order kinetics. If the initial concentration of chemical B is 1.2 M and…

A: The answer is given as follows

Q: of

A: Using first order integrated equation, k • t = 2.303 • log( [A]o / [A] ) k • 1.35 • 10^2 s = 2.303…

Q: . For the following consecutive first order reactions K =2.0s- K =2.0s →Y the time (in seconds)…

A: Here it is given a first order consecutive reaction.we will find the time required for Y to reach…

Q: After 74.0 min, 24.0% of a compound has decomposed. What is the half-life of this reaction assuming…

Q: A certain first-order reaction is 43.5 percent complete in 6.90 min at 25°C. What is its rate…

Q: What is the reactant concentration after 78.9 seconds for a second order reaction with a half-life…

Q: if the initial concentration of both the reactant following second order reaction kinetics are the…

A: Initial concentration (A0) = 100 (value is not given so we will assume concentration is 100) Final…

Q: Calculate the half life, in seconds, for a first order reaction with an initial concentration of…

A: Given : Initial concentration of reactant = 0.104 M Order of reaction = 1 And rate constant of…

Q: What is the half-life for a first order reaction if the initial concentration of reactant is 1.25M…

A: Given that it is a first-order reaction. Initial concentration [Co]= 1.25M Final concentration[C] =…

Q: The reaction of C4H Cl with water is a first-order reaction. The reaction half-life is 340 s. If the…

A: The given problem can be solved by using the formula for the first order given below as; First…

Q: (a) Derive the equation for (integral form) 1st order reaction and show that change of units of…

A: First, we need to derive the 1st order equation. The derivation is shown in step 2.

Q: A first order reaction has a rate constant of 0.00318 min1. what is the half-life of the reaction?

A: Given, rate constant of first order reaction =0.00318 min-1we are asked to calculate the half-life…

Q: The rate constant for the first-order conversion of A to B is 3.33 hr-1. How much time will be…

A: Given K(rate constant) = 3.33/hr Time required for reaching 75% of original value=?

Q: It takes 5 minutes to reduce a certain reactant to 75% its original value, following a third-order…

Q: How long would it take for a first-order reaction with a rate constant of5.30 X 10-4 s-1 to reach…

Q: A certain first-order reaction has a rate constant of 2.50×10−3 s^−1. How long will it take for the…

Q: For the first order reaction, the initial concentration of A= .4 M. What is the half life of the…

A: when the rate of the reaction depends only on the concentration of the reactant and its power is one…

Q: The rate constant for a first order reaction is 60 s-1. How much time will it take to reduce the…

A: The rate constant of the first order reaction is given by, kt=log[A]0[A] where k is the rate…

Q: For a certain first order reaction, 20 % of the reactant is consumed after the 90. min. How long…

Q: After 51.0 min, 16.0% of a compound has decomposed. What is the half-life of this reaction assuming…

Q: Calculate the rate constant (in units 1/M•min) for a second order reaction with a half life of 70.1…

A: Given :- half life (t1/2) = 70.1 min (2nd order reaction) Initial concentration [A]0 = 0.556 M To…

Q: After 48 seconds, 10.% of reactant has reacted. If the reaction is a 1st order reaction, the special…

A: Given that 10% of reactant has reacted. It implies that if 100% of reactant is present initially,…

Question

Time and concentration data were collected for the reaction
0.52
0.48
A
→ products
0.44
t (s)
[A] (M)
0.40 -
0.52
20
0.43
2 0.36
40
0.35
0.32 -
60
0.29
0.28
80
0.23
0.24
100
0.19
0.20
The blue curve is the plot of the data. The straight orange line
is tangent to the blue curve at t = 40 s.
0.16
0 10 20 30 40 50 60 70 80 90
t (s)
Approximate the instantaneous rate of this reaction at time
t = 40 s.
instantaneous rate:
M/s
[A] (M)

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
For the reaction 2N2O5(g)4NO2(g)+O2(g) the following data were collected, where Rate=[N2O5]t Time (s) T = 338 K [N2O5] T=318K [N2O5] 0 1.00 101 M 1.00 101 M 100. 6.14 102 M 9.54 102 M 300 2.33 102 M 8.63 102 M 600. 5.41 1O3 M 7.43 102 M 900. 1.26 1O3 M 6.39 102 M Calculate Ea for tills reaction.
List at least four experimentally determined parameters that you, an experimenter, can define when exploring the hydrolysis of ethyl benzoate by aqueous sodium hydroxide.
Consider the reaction data. A⟶productsA⟶products ? (?)T (K) ? (?−1)k (s−1) 275275 0.3800.380 675675 0.7470.747 a)What two points should be plotted to graphically determine the activation energy of this reaction? To avoid rounding errors, use at least three significant figures in all value x1=? x2=? y1=? y2=? b)Determine the rise, run, and slope of the line formed by these points. c)What is the activation energy of this reaction?
A student collects the following data: Time (s) [X] mol*L-1 0 0.0200 800 0.0101 1600 0.0067 2400 0.0051 3200 0.0042 Explain how the student can determine if the reaction is a zero, first, or second order reaction by looking at it graphically. In your explanation, justify your response by contrasting all possible data plots.
for the reaction A -> B where at t=0, t=20s, t=40s A=0.30 mol A=1.0mol A=0.54mol B= 0.46mol B=0.70mol calculate tge average appearance of B over the time interval from 0 -> 40s
Consider the experimental data collected for the following chemical reaction: 2H2(g) + 2NO(g) → N2(g) + 2H2O(g) Trial Initial [H2] (mol/L) Initial [NO] (mol/L) Rate of Reaction (mol/L∙s) 1 0.031 0.0025 2.0 x 10-3 2 0.062 0.0025 4.0 x 10-3 3 0.031 0.0050 8.0 x 10-3 4 0.062 0.0050 1.6 x 10-2 Which action will have more effect on the rate of this reaction; changing the concentration of H2(g) or that of NO(g)? Explain your reasoning by considering the orders of reactants and writing the corresponding rate law equation.
determine: 1)reaction order 2)value of K
Use Cleland notation to describe Ordered and Random sequential reactions and a Ping Pong reaction.
For A⟶products, time and concentration data were collected and plotted as shown. [A] (M) t (s) 0.750 00.0 0.596 30.0 0.473 60.0 0.376 90.0 Determine the reaction order, the rate constant, and the units of the rate constant. order= k= units
Consider the reaction data. A⟶productsA⟶products T (K)T (K) k (s−1)k (s−1) 325325 0.3770.377 675675 0.7230.723 What two points should be plotted to graphically determine the activation energy of this reaction? To avoid rounding errors, use at least three significant figures in all values. x1= x2= y1= y2= Determine the rise, run, and slope of the line formed by these points. rise: run: slope: What is the activation energy of this reaction?
The activation energy for the reaction 2 NO2(g) → 2 NO(g) + O2(g) is 111 kJ mol- 1. What proportion of the collisions between NO2 molecules have enough energy toresult in reaction when the temperature is (a)20 oC. (b)200 °C? Use collision theory to estimate the pre-exponential factor for the reaction. The experimental value is 2 x 109 dm3 mol-1 s-1. Suggest a reason for any discrepancy.