A reaction has a rate constant of k = 2.55 s 1. What is the overall reaction order?Equations.Rate = k[A][B]²k₁[A₂] = k-1[A]²-EaIn[A] = -akt + ln[A]ok = Ae RTIn 2Ea=t₁/2 =In k = ln A -akRT11Ea= 2kt +[A][A].In (1/²) = 5/²2 (1/17 - ²2/1)RT₁T21=2k[A].t1/21st order2nd order3rd orderO4th orderNone of the above.

Given : for a reaction the value of rate constant (K) = 2.55 s-1 To determine : overall reaction…

Answered: A reaction has a rate constant of k =…

Science

Chemistry

A reaction has a rate constant of k = 2.55 s¹. What is the overall reaction order? S

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: estimate the value of the rate constant k

A: Recall the given reaction, [A] (M)Initial rate…

Q: The following data are for the gas phase decomposition of dimethyl ether at 500 °C. CH3OCH3(g) ·…

A: A) For the given reaction- CH3OCH3 (g) -----> CH4 (g) + H2 (g) + CO (g)

Q: A(g) + B(g) C(g) The rate law for the above reaction is: -d[A]/dt = k[A][B] The rate constant is…

Q: When the reaction of 2 NO2(g) → N2O4(g) goes through the second order kinetics. Find the…

A: Given- Reaction 2 NO2(g) → N2O4(g) Order of reaction = 2 Initial concentration of NO2 = 1.66 M Final…

Q: N₂O5(g) decomposes according to the following reaction: 2N2O5(g) → 4NO₂(g) + O₂(g) The…

A: Intermediates are those species which are not present neither before the start of the reaction nor…

Q: Calculate the rate constant, k, for a reaction at 67.0 °C that has an activation energy of 77.5…

Q: The reaction AB(aq) - has a rate constant of 0.0118 M-1.s-'at 25.0°C. A reaction ves- A(g) + B(g) is…

A: The given reaction is second-order hence rate law: Reaction: Data are given: The initial…

Q: A reaction has a rate constant of 0.00205 s–1. What is the half-life (in min to two decimal places)…

Q: Consider the following reaction at 308 K: 2 A(g) + B(g) → C(g) + D (g) where rate = k[A][B]2. An…

A: where rate = k[A][B]2. An experiment was performed for a period of time with [A]0= 1.386 M and [B] =…

Q: The activation energy for a reaction is changed from 184 kJ/mol to 59.0 kJ/mol at 600. K by the…

A: Activation energy means amount of energy that must be provide to a reactant so that it change into…

Q: The rate constant for the reactionBr(g)+O3(g)---->BrO(g)+O2(g)was determined at the four…

A: To plot the graph the values of 1/T and ln k is determined.

Q: The reaction AB(aq)A(9)+B(g) is second order in AB and has a rate constant of 0.0140 L- mol-.s' at…

A: k = 0.0140 L.mol-1.s-1 [AB]o = 0.188 mol.L-1

Q: Consider the hypothetical first-order reaction A products, k = 0.0275 s-1. If the initial…

Q: Consider the reaction described by the equation C,H,Br, (aq) + 3I¯(aq) → C,H,(g) + 2 Br¯(aq) + I5…

A: Given C2H4Br2 + 3I- → C2H4 + 2 Br- + I3-( aq ) Rate( R ) = K [ C2H4Br2 ] [ I- ] Rate…

Q: Initial-rate data at a certain temperature is given in the table for the reaction C₂H₂Cl(g) →→→…

Q: What is the half-life of this reaction at 1000°C?

Q: The rate constant for the reaction is 0.770 M−1⋅s− at 200 ∘C. A⟶products If the initial…

A: Given the rate constant is 0.770 M-1 s-1, from the unit of rate constant it is clear that reaction…

Q: write the rate law for the following reaction: H2S(g)+Cl2(g)-->S(s)+2HCl(g) represent the order as…

A: Order of the reaction tells about the rate of the reaction and the concentration of all the species…

Q: tration of the reactant. Which of the following is most likely to be true of this reaction? he…

A: Zero-order reactions take place when a material that is required for the reaction to proceed, such…

Q: A reaction has a rate constant, k = 1.29 s-1. What is the half-life (seconds) when the initial…

Q: Consider the reaction A⟶ Products. The rate law for this reaction is rate = k[A] where k=2.90 ×10-4…

A: Given, k=2.90 ×10-4 s-1 [A] = 0.0500 M

Q: SO2Cl2 (g)SO2 (g) + Cl2(g). The reaction is initiated, and the following data are obtained.…

Q: 1. HS (aq) + H₂O(g) ←➜ S²¯(aq) + H₂O*(aq) Write a rate law for the reaction given the reaction is…

A: First we need to determine overall order of the reaction.

Q: The rate constant for a certain reaction is k = 1.60×10-³ s-¹. If the initial reactant concentration…

Q: Calculate the rate constant, ?k, for a reaction at 69.069.0 °C that has an activation energy of…

Q: The rate constant for the reaction is 0.130 M−1⋅s−1 at 200 ∘C A⟶products If the initial…

A: Rate is the speed at which a reaction takes place. The rate of appearance of the product equals to…

Q: reaction has a rate constant, k = 0.0866 M-1 s-1. What is the half-life (seconds) when the initial…

A: k = 0.0866 M-1 s-1 [Ao] = 4.27 M

Q: The rate constant for a certain reaction is k = 8.80×10−3 s−1 . If the initial reactant…

A: From the unit of rate constant we can say that it is first order equation

Q: The hydrolysis of sucrose (C12H22O11)(C12H22O11) into glucose and fructose in acidic water has a…

A: GIVEN: rate constant = 1.8 * 10 - 4 s-1 Volume of sucrose= 2.65L Molarity of sucrose = 0.150 M Time…

Q: A reaction has special rate constant k = 0.125 1/M•sec, if the reactant has initial concentration…

A: Given: Rate constant = 0.125 1/(M•sec) initial concentration [A]0 = 8.0 M time = 19 seconds We…

Q: Determine the rate law and the value of k for the following reaction using the data provided. 2…

A: The kinetics data given is,

Q: The rate constant at a given temperature for the reaction A2 B is 0.0145 s1. What is the…

A: Given reaction is A ---------> 2 B Rate constant= 0.0145 s-1 Initial concentration of A = 2.6 M…

Q: The following dissociation reaction has an activation energy of 262 kJ/mol C4H8 (g) 2 C₂H4 (g) At…

Q: The rate constant for a certain reaction is k = 7.60×10−3 s^-1 . If the initial reactant…

Q: The rate constant for a certain reaction is k = 5.10×10−3 s−1 . If the initial reactant…

A: The objective of the question is to find the concentration of the reactant after 20.0 minutes given…

Question

A reaction has a rate constant of k = 2.55 s 1. What is the overall reaction order?
Equations.
Rate = k[A][B]²
k₁[A₂] = k-1[A]²
-Ea
In[A] = -akt + ln[A]o
k = Ae RT
In 2
Ea
=
t₁/2 =
In k = ln A -
ak
RT
1
1
Ea
= 2kt +
[A]
[A].
In (1/²) = 5/²2 (1/17 - ²2/1)
RT₁
T2
1
=
2k[A].
t1/2
1st order
2nd order
3rd order
O4th order
None of the above.

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 1 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

Calculate the rate constant, k, for a reaction at 57.0 °C that has an activation energy of 79.0 kJ/mol and a frequency factor of 6.79 x 1011 s-1. k =
Calculate the rate constant, k, for a reaction at 61.0 °C that has an activation energy of 78.9 kJ/mol and a frequency factor of 2.66 x 101 s-1. k =
Consider the following reaction at 300. K: A B + 2C. Determine the order of the reaction with respect to A if the experimental rate law is: Rate O-1 O-1/2 0 O 1/2 1 3/2 [A]²[B] [9] 02
The reaction C,H,(g) → 2 C,H,(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 × 10-8 s-'. What is the value of the rate constant : 775.0 K? k = ?
The reaction: C4H8(g)⟶2 C2H4(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1×10−8 s−1. What is the value of the rate constant at 860.0 K?
The following data were obtained for the reaction of carbon monoxide with chlorine, producing phosgene, COCl2, a highly toxic gas CO(g) + Cl2(g) → COCl2(g) From the following data, obtained at 360 K, determine: a) The order of the reaction, and the reaction rate law b) The value of the reaction rate constant, k c) The initial reaction rate for the formation of COCl2 when the concentration of CO is 0.30 M and that of Cl2 is 0.40 M The following data were obtained for the reaction of carbon monoxide with chlorine, producing phosgene, COCl2, a highly toxic gas CO(g) + Cl2(g) → COCl2(g) From the following data, obtained at 360 K, determine: a) The order of the reaction, and the reaction rate law b) The value of the reaction rate constant, k c) The initial reaction rate for the formation of COCl2 when the concentration of CO is 0.30 M and that of Cl2 is 0.40 M The following data were obtained for the reaction of carbon monoxide with chlorine, producing phosgene, COCl2, a highly toxic…
The first-order rate constant for the decomposition of C2H5Cl, C2H5Cl(g) C2H4(g) + HCl(g) at 27 oC is k = 7.27e-30 s-1. Suppose we start with 0.0845 mol of C2H5Cl in a volume of 4.9 L. How many moles of C2H5Cl will remain after 1.24e+27 min?
The rate constant for the reaction is 0.450 M−1⋅s−1 at 200 ∘C. A⟶products If the initial concentration of A is 0.00610 M, what will be the concentration after 405 s?
A particular first-order reaction has a rate constant of 1.35 x 102 s at 25.0 ° C. What is the magnitude of k at 55.0°C if Ea = 55.5 kJ/mol. 1.05 103 2.67 1065 277 1.35 102 1.65 104
How can measurements of reaction half-lives be used to determine the order of a reaction?
Define rate constant (K).
Calculate the rate constant, k, for a reaction at 54.0 °C that has an activation energy of 86.9 kJ/mol and a frequency factor of 8.84 x 10'1 s-1. k =