A reaction has a rate constant of k = 2.55 s¹. What is the overall reaction order?Equations:Rate = K[A][B]²kı[A2] = k-1[A]²-EaIn[A] = -akt + In[A]ok = Ae RTIn 2Eat₁/2 =Ink In A-akRT11Ea/1= 2kt +[A]=[A]oIn (*) - (-+)RT₁ T₂1t1/22k[A]oO1st order2nd order3rd order4th orderO None of the above.

Given :- rate constant (K) = 2.55 s-1 To determine :- overall reaction order

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?

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

Similar questions

The rate constant for a certain reaction is k = 5.10×10−3 s−1 . If the initial reactant concentration was 0.950 M, what will the concentration be after 20.0 minutes?
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 =
When designing a consumer product, it is desirable for it to have a two-year shelf life. Often this means that the active ingredient in the product should not decrease by more than 5% in two years. If the reaction is first order, and the rate constant is: k = 2.56 × 10-2 yr 1, determine the half-life of an active ingredient that has a shelf life of 2.00 years. The half-life of an active ingredient is i yr.
Cyclopropane (C3H6) reacts to form propene (C3H6) in the gas phase. The reaction is first order in cyclopropane and has a rate constant of 5.87 * 10 - 4>s at 485 °C. If a 2.5-L reaction vessel initially contains 722 torr of cyclopropane at 485 °C, how long will it take for the partial pressure of cyclopropane to drop to below 1.00 * 102 torr?
Consider a decomposition reaction that occurs via the following balanced chemical equation: AB2 → AB + B This reaction is first order with k = 7.7 x 10-7 s-1. What is the half-life (t1/2) of this reaction when the temperature is 1000.°C, and the initial concentration of AB2 is 0.269 M? Express your answer in units of seconds.
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of ·0.0081Ms−1 2HI(g)→H2(g)+I2(g) Suppose a 4.0L flask is charged under these conditions with 400.mmol of hydrogen iodide. After how much time is there only 200.mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
A possible reaction for the degradation of the pesticide DDT to a less harmful compound was simulated in the laboratory. The reaction was found to be first order, with k = 2.47 x 10-8 s-1 at 25°C. What is the half-life for the degradation of DDT in this experiment, in years? (1 year = 365 days)
A possible reaction for the degradation of the pesticide DDT to a less harmful compound was simulated in the laboratory. The reaction was found to be first order, with k = 2.55 x 108 s at 25°C. What is the half-life for the degradation of DDT in this experiment, in years? (1 year = 365 days) Round your answer to 2 decimal places.
Consider the following reaction: A + B + C → D The rate law for this reaction is as follows: [A][C]* Rate = k [B]L/2 Suppose the rate of the reaction at certain initial concentrations of A, B, and C is 1.17x10-2 mol · L-ls¬1. Part A What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled? Templates Symbols uado redo reset keyboard shortcuts help Rate = mol · L-!s-1
The rate constant for a certain reaction is k = 2.00×10−3 s−1 . If the initial reactant concentration was 0.950 MM, what will the concentration be after 16.0 minutes?
Using the following reaction: A + 2B → C + D Describe how the rate of disappearance of B will compare to the rate of appearance of C at the start of a reaction. It is determined that A and B are first order reactants. Explain how you would write out the rate law and units of the equilibrium constant with respect to the equation above.
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 =