2. (a) You study the effect of temperature on the rate of two reactions and graph the natural logarithm (In) of the rate constant for each reaction as a function of Explain, with the aid of diagrams and equations, how the two graphs compare if (i) The activation energy of the second reaction is higher than the activation energy of the first reaction but the two reactions have the same frequency factor. (ii) The frequency factor of the second reaction is higher than the frequency factor of the first reaction but the two reactions have the same activation energy.

2. (a) You study the effect of temperature on the rate of two reactions and graph the natural logarithm (In) of the rate constant for each reaction as a function of Explain, with the aid of diagrams and equations, how the two graphs compare if (i) The activation energy of the second reaction is higher than the activation energy of the first reaction but the two reactions have the same frequency factor. (ii) The frequency factor of the second reaction is higher than the frequency factor of the first reaction but the two reactions have the same activation energy.

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

Related questions

Q: (a) Explain the following terms :(i) Order of a reaction(ii) Molecularity of a reaction(b) The rate…

Q: The reaction 2 ClO2(aq) + 2 OH- (aq)--->ClO3- (aq) +ClO2- (aq) + H2o(l) was studied with the…

Q: Consider the following reaction: 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) (a) The rate law for this…

A: The reaction taking place is given as, => 2 NO (g )+ 2 H2 (g) ↔ N2 (g) + 2 H2O (g) Given: Order…

Q: (c) The rate constant for a certain reaction is 2.52 x 10 *s' at 463K and 6.30 x 10°s at 503 K.…

A: The question is based on the concept of chemical kinetics. we have been given rate constant values…

Q: The water in a pressure cooker boils at a temperature greater than 100°C because it is under…

A: i) To determine the activation energy for the reaction associated with the cooking of food. Given:…

Q: A reaction performed at 1.00 °C exhibits a rate constant of 1.115 s–1. What temperature (in °C to…

Q: |CE] (M) 0.0100 Еxperiment |NO] (M) Rate (M/s) 1 0.0300 3.4 x 104 2 0.0150 0.0100 8.5 x 10-5 3…

A: Rate constant can be find by finding order of equation. Then Putting any experimental values give…

Q: (a) The gas-phase decomposition of SO2Cl2, SO2Cl2(g)------->SO2(g) + Cl2(g), is first order in…

A: The term first order reaction is defined for those reactions which proceed at a rate that has a…

Q: The table at right shows the rate constants for the rearrangement of methylisonitrile at various…

A: (a) Activation energy for the reaction is calculated as follows, Consider any two values of…

Q: 12. (a)A chemical reaction has an activation energy of 12.0 kJ/mol at 298.K. What is the fraction of…

A: Activation energy is 12 KJ/mol Temperature is 298 K We have to calculate fraction of collision that…

Q: A particular second-order reaction has a rate constant of 2.4 x 10–6 M–1 s–1 at 575 K and 6.0 x 10–5…

Q: A catalyst decreases the activation energy of a particular exothermic reaction by 33 kJ/mol, to 25…

A: Activation energy of catalyzed reaction = 25 kJ/molActivation energy difference between the…

Q: The combustion of ethane (C₂H6) is represented by the equation: 2C₂H6(g) +70₂(g) 4CO₂(g) + 6H₂O(l)…

A: for the given reaction, it is understood from the question that we have to identify the correct…

Q: This is based on the binding of glucose to hexokinase. The enzyme concentrations are constantly…

A: Solution -

Q: 2a) Briefly explain, in your own words, the difference between the "activation energy" of a reaction…

A: (2a) Activation energy of a reaction Activation energy is introduced by a scientist named Svante…

Q: Molecular iodine, I2(g), dissociates into iodine atoms at 625 Kwith a first-order rate constant of…

A: Half-life is the time required for the reaction to be half completed. It is denoted by t1/2 . For a…

Q: 2) Acetoacetic acid, CH3COCH2COOH, a reagent used in organic synthesis, decomposes in acidic…

A: Given, First order reaction. Half-life = 144 minutes

Q: n order to be effective, a certain drug must be at amountgreater than 10 mgin the body.The drug is…

Q: Hydrogen peroxide decomposes spontaneously to yield water and oxygen gas according to the reaction…

Q: (a) In the reaction mechanisms given, there are some chemical species which will get produced in one…

Question

2. (a) You study the effect of temperature on the rate of two reactions and graph the natural logarithm (In)
of the rate constant for each reaction as a function of Explain, with the aid of diagrams and
equations, how the two graphs compare if
(i) The activation energy of the second reaction is higher than the activation energy of the first reaction
but the two reactions have the same frequency factor.
(ii) The frequency factor of the second reaction is higher than the frequency factor of the first reaction
but the two reactions have the same activation energy.

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 3 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

The activation energy for the isomerization reaction CH3NC(g) → CH3CN(g) is 161 kJ mol−¹, and the reaction rate constant at 600 K is 0.41 s¯¹. (a) What is the value of the pre-exponential factor A for this reaction? (b) What is the value of the rate constant of the reaction at 1000 K?
Which of the following is correct? (A) The activation energy changes when temperature changes. (B) The Arrhenius equation only applies to 1st order reactions. (C) The rate constants at higher temperatures are ALWAYS larger than at low temperatures for the same chemical reaction. (D) The rates of reaction at higher temperatures are ALWAYS larger than at low temperatures for the same chemical reaction.
The rate constant of the elementary reaction BH, (aq) + NH (aq) → BH;NH3 (aq) + H2 (g) is k = 1.94 x 10-4L mol¯' s-' at 30.0°C, and the reaction has an activation energy of 161 kJ mol. (a) Compute the rate constant of the reaction at a tem- perature of 40.0°C. (b) After equal concentrations of BH (aq) and NH, (aq) are mixed at 30.0°C, 1.00 × 10ª s is required for half of them to be consumed. How long will it take to consume half of the reactants if an identical experi- ment is performed at 40.0°C?
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.
Which of the following is always true about a unimolecular reaction? (A) The activation energy is twice that of a unimolecular reaction. (B) The rate of the reaction doubles when the concentration of the reactants doubles. (C) If the temperature is doubled, the reaction rate doubles. (D) A larger molecule breaks down into two smaller molecules. (E) Two particles must collide together for the reaction to occur.
Determine which of the two diagrams here (both for the same reaction) involves a catalyst, and identify the activation energy for the catalyzed reaction: 100 100 90 80 70 60 90 80 70 60 50 40 30 50 40 30 20 10 20 10 Extent of reaction Extent of reaction (a) (b) Energy (kJ) Energy (kJ)
5. The collision theory of reaction rates states that the rate of a reaction depends on the number of collisions between mol- ecules, the average energy of the collisions, and the effectiveness of the collisions. (a) How does temperature affect each of these factors in collision theory? (b) Does the effect of temperature on the reaction rate support the collision theory of reaction rates? Explain.
A number of reactions that take place on the surfaces of cata lysts are zeroth order in the reactant. One example is the decomposition of ammonia on hot tungsten. In one experiment. the partial pressure of ammonia decreased from21 kPa to 10 kPa in 770 s. (a) What is the rate constant for the zeroth-order reaction? (b) How long will it take for all the ammonia to disappear?
Given the following values of the enthalpy (DH) and activation energy (Ea) of four different reactions, identify an exothermic reaction that would exhibit the fastest rate at 298 K. (Assume that all reactants have the same initial concentration and the same Arrhenius frequency factor A in k = Ae-Ea/RT). (A) DH = +45 kJ/mol; Ea = 75 kJ/mol; (B) DH = +35 kJ/mol; Ea = 65 kJ/mol; (C) DH = -35 kJ/mol; Ea = 75 kJ/mol; (D) DH = -45 kJ/mol; Ea = 65 kJ/mol;
a)A nickel catalyst is commonly used in the hydrogenation of ethylene. If the initial concentration of ethylene is 2.75 mol·L−1 and the rate constant for the reaction is 0.0018 mol·L−1·s−1, what is the rate of reaction if it follows a zero-order reaction mechanism? Express your answer to two significant figures. b)Determine the half-life for the reaction in Part B. Express your answer to two significant figures.
Consider the following reaction: 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g)(a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). What is the rate law for this reaction?(b) If the rate constant for this reaction at a certain temperature is 8.80e+03, what is the reaction rate when [HBr(g)] = 0.00429 M and [O2(g)] = 0.00758 M?Rate = _______ M/s.(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00858 M while the concentration of O2(g) is 0.00758 M?Rate = _______ M/s
1. (a) Show that decomposition of the organic compound 1,3-pentadiene is a second-order reaction and determine the rate constant. The concentration of 1,3-pentadiene was measured as a function of time. The data are as follows: (b) What is the value of the rate constant for the decomposition of 1,3-pentadiene.(c) What is the initial concentration for the reaction? Report to 3 significant figures.(d) What is the concentration of 1,3-pentadiene after 3.750 x10^3 s? Time(s) [1,3-pentadiene] (M) 0 .480 1000 .179 2000 .110 3000 .0795 4000 .0622 5000 .0510