Consider the hypothetical reactionA+B+2C 2D+3Ewhere the rate law isAA)AtRate=-KA][B]¹An experiment is carried out where[A]1.0 x 10 M.(B) -pscopy-CHMIa. Calculate the value of k for this reaction.k=L' mol-1[Review Topical8.0 M, and(C2.0 M. The reaction is started, and after 7.0 seconds, the concentration ofA is3.8 x 10 M.b. Calculate the half-life for this experiment.Half-lifec. Calculate the concentration of A after 19.0 seconds.Bubmit AnswerConcentration =Md. Calculate the concentration of C after 19 seconds.Concentration -MRatry Entire GroupGOWL21 Online teaching and learning resource from Cengage Learningmore group attemptingReferences)

Given, Reaction : A+2B+2C→2D+3E rate law : rate=-∆A∆t=k[A][B]2

Consider the hypothetical reaction A+B+2C 2D+38 where the rate law is AA) At Rate= -A[AB An experiment is carried out where [A-1.0 x 10 M. [B) - 8.0 M, and C-2.0 M. The reaction is started, and after 7.0 seconds, the concentration of A is 3.8 x 10 M. a. Calculate the value of k for this reaction. b. Calculate the half-life for this experiment. Half-life= c. Calculate the concentration of A after 19.0 seconds. Concentration - M d. Calculate the concentration of C after 19 seconds. Concentration - M

Consider the hypothetical reaction A+B+2C 2D+38 where the rate law is AA) At Rate= -A[AB An experiment is carried out where [A-1.0 x 10 M. [B) - 8.0 M, and C-2.0 M. The reaction is started, and after 7.0 seconds, the concentration of A is 3.8 x 10 M. a. Calculate the value of k for this reaction. b. Calculate the half-life for this experiment. Half-life= c. Calculate the concentration of A after 19.0 seconds. Concentration - M d. Calculate the concentration of C after 19 seconds. Concentration - M

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

Reaction rate for the chemical reaction 2A + B → A2B Select one: a. V = KCA .CB b. V = KCB c. V = KCA2 d. V = KCA2 .CB
k=? k=?
PS. this is not graded.
Each step represents an elementary reaction. Step1. A + 2B + C (fast equilibrium, k and k.j) Step2. C +D → E (slow, k2) a. Find the balanced equation. *b. Order the species as 'Catalyst', 'Intermediate', 'Reactant' or 'Product'. *c. Find the rate-determining step (RDS) and express the rate law. d. Use the Pre-Equilibrium Approximation to obtain the rate law. *e. Use the Steady-Sate Approximation to obtain the rate law.
Hw.38.
ONLY LOOKING FOR THE ANSWER TO PART B. I already got part one!
What is the concentration of A after 30.5 minutes for the reaction A → Products when the initial concentration of A is 0.750 M? (k = 0.0451 M⁻¹min⁻¹)
The elementary reaction 101 4 2H₂O(g) = 2H₂(g) + O₂(g) proceeds at a certain temperature until the partial pressures of H₂O, H₂, and O₂ reach 0.0700 atm, 0.00350 atm, and 0.00300 atm, respectively. What is the value of the equilibrium constant at this temperature? Kp = O R 01 F % 5 1 T a G 6 24 1 & Y H 7 U 8 J 144 ( 9 K BO O O ☐ L Resources DDI P { 2. ✈ ? 59°F [ insert pause prt sc Hint 10/1/2022 backspace delete home enter pg ur T shift in er
Rate = k [A] [B]² Overall reaction order would be A. 0 В. 1 С. 3 D. 2 What is the connection between rate and temperature ? A. There is no connection between the two B. Rate is indirectly connected to temperature C. Rate is directly related to temperature in exothermic reactions and indirectly related to temperature in endothermic reactions D. Rate is directly connected to temperature E. Rate is indirectly related to temperature in exothermic reactions and directly related to temperature in endothermic reactions
For the exothermic reaction 4 NH3(g) +7 02(g)- => 4 NO2(g) + 6 H20(g) which change will increase the quantity of NO2 in the mixture? O A. increasing temperature OB. decreasing container volume OC. adding Ne(g) O D. adding H20(g) O E. adding a catalyst
The proposed mechanism for a reaction is NO + 03 2 N03 0 Fast pre-equilibrium NO3+0 N02 +02 Slow Which of the following would be a rate law for the reaction? OA. rate k[NO][03] B. rate k[O3] OC. rate = k[NO] O D. rate = k[O][NO3] E. rate k[NO2][02]
Given the intermediate step for the reaction: SO + O2 > SO2 + O Which collision path would be an "effective" collision? A. SO- O=O or B. O=O- SO Then explain why you selected the choice.