**Chemical Reaction Rate Law Problem**The rate law for the reaction \(A + B \rightarrow C\) was found to be:\[ \text{rate} = k[A][B] \]One experimental trial with the concentrations \([A] = 0.26 \, \text{M}\) and \([B] = 0.13 \, \text{M}\) had an initial rate of product formation of \(0.36 \, \text{M/s}\).**Question:**What is the value of the rate constant \(k\) for this reaction?**Answer:**Enter your answer as 0.0035 with no units. Use 2 significant digits.**Answer:** [ ]

Answered: Image /qna-images/answer/144597d7-f9b9-4291-a943-d3167a602e35.jpg

The rate law for the reaction A + B → C was found to be rate = k[A][B]. One experimental trial with the [A] = 0.26 M and (B] = 0.13 M had an initial rate of product formation of 0.36 M/s. What is the value of the rate constant for this reaction? Enter your answer as 0.0035 with no units. Use 2 significant digits. Answer:

The rate law for the reaction A + B → C was found to be rate = k[A][B]. One experimental trial with the [A] = 0.26 M and (B] = 0.13 M had an initial rate of product formation of 0.36 M/s. What is the value of the rate constant for this reaction? Enter your answer as 0.0035 with no units. Use 2 significant digits. Answer:

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

Dinitrogen pentoxide rapidly decomposes in the atmosphere with the rate law noted. 2 N₂O5 (g) → 4 NO2 (g) + O₂(g) rate= (5.85 × 10-³s-¹) [N₂05] S How long does it take for sample to decompose from an initial concentration of 0.750M to0.211M ? Answer formatting tip: enter the reaction time using three significant figures; omit the units of s.
In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H2(g) + ½ I½(g) the concentration of HI was followed as a function of time. It was found that a graph of [HI] versus time in seconds gave a straight line with a slope of -1.91×10-4 Ms and a y-intercept of 0.235 M. Based on this plot, the reaction is reaction is order in HI and the rate constant for the Ms!
please answer prt 4 and 5 with the correct sig figs
We are determining the rate law equation for a reaction A + B + C > ABC in which a dramatic and instant color change tells us that reactants are used up and product is formed. (Concentrations used in all experiments are [A] = 2.0M, [B] = 1.0M and [C] = 3.0M) This is the data for questions 19 through 22: Volume of Volume of water, C, Volume of Volume of Time from mixing to dramatic color А, B, ml change, sec ml ml ml 1.0 1.0 1.0 97.0 16 1.0 1.0 2.0 96.0 8 19) Which reactant concentration have we changed? a) A b) B c) C d) no reactant concentrations changed
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E=67.0 kJ/mol. If the rate constant of this -1 −1 reaction is 3.9 M •S at 99.0 °C, what will the rate constant be at 178.0 °C? Round your answer to 2 significant digits. - 1 -1 ☐ k = M • S ? x10 X Ś
Question 23 Identify the rate-determining step based on the rate law you found in question 23. Given these data for the acid-catalyzed reaction in question 22, fınd the rate law. 0–H [RCOOH], M [R'OH], M (HA], M Initial Rate, Ml·min' || R-c-o–H 0.35 0.35 0.50 4.60 0.50 + HA - R-Ć+ k2 0.62 0.35 8.14 A- 0.35 0.81 0.50 10.6 0.35 0.50 0.75 9.84 0–H Group 1 Rate = k[RCOOH][R'OH] 0–H 0–H k3 O Rate = k[RCOOH][R'OH][HA] R-C+ A + R -0–H R—С—0—Н Rate = k[RCOOR']/{[RCOOH][R'OH]} k4 0–H R'-o+ A- Rate = k[R'OH] Group 2 H Rate = k[RCOOH] 0–H k5 R—С—0—н R-C-0–R' + H2O + HA R-o+ A- Group 3 H. Step 2 or Step 3 Step 1 or Step 2 Step 1 or Step 3 Step 2 Step 1
Show your work please, thank you!
Help with the question on the right Question 23 Identify the rate-determining step based on the rate law you found in question 23. Given these data for the acid-catalyzed reaction in question 22, find the rate law. 0–H (RCOOH), M [R'OHJ, M (HAJ, M Initial Rate, M-min"' - R-C+ k2 R С—0—Н + HA A- 0.35 0.35 0.50 4.60 0.50 0.62 0.35 0.35 8.14 0.81 0.50 10.6 0.35 0.50 0.75 0–H 9.84 Group 1 0–H 0–H k3 Rate = k[RCOOH][R'OH] R-Ć+ A- R 0–H R—С—0—Н + Rate = k[RCOOH][R'OH][HA] k4 0–H R-ó+ A- Group 2 Rate = k[RCOOR']/{[RCOOH][R'OH]} H Rate = k[R'OH] 0–H Rate = k[RCOOH] k5 R- C-0–R' R-C-0–H + H,о + НА R-o+ A- Group 3 Step 2 or Step 3 O Step 1 or Step 2 Step 1 Step 3 Step 2 Step 1
60 QUESTION 13 The following graphs can be used for the questions that follow: 00 B0 00 Seris 1 02 time(min) D2 -D4 y = -0.0358x + 0.1058 Liner (Serive t) -18 time(min) The decomposition reaction of NO 2 is important in atmospheric chemistry. The reaction 2NO 2(g) → 2NO(g) + O 2(g) is second order with respect to NO 2. How can the rate constant be determined? A plot of 1/[NO2] versus time will be linear with a slope of -k. A plot of 1/[NO2] versus time will be linear with a slope of k. A plot of [NO2] versus time will be linear with a slope of -k. A plot of In[NO2] versus time will be linear with a slope of -k. Click Save and Submit to save and submit. Click Save All Answers to save all answers. MacBook Air DD F8 F3 F4 F5 F1 %23 24 2 4. 7.
For the reaction: IO3 (aq) + 5 I (aq) + 6 H* (aq) + 3I2 (aq) + 3 H2O (l) the reaction rate of I° (aq) is 2.6 x 10-3 M/s Calculate the rate at which (ac) is formed.
Which equation best describes the average rate for the reaction shown? A(aq) + B(aq) → C(aq) + D(aq) Multiple Choice rate = [C][D] [A][B] rate = +Δ[B]/Δt rate = –Δ[C]/Δt rate = –Δ[A]/Δt rate = [A][B] [C][D]
2:26 ◄ Bartleby Experiment Determine the rate law for the following reaction using the experimental data given below. 2NO+O₂ → 2NO2 1 2 3 O rate=k[NO][0₂] O rate=k[NO]²[0₂] O rate=k[NO]²[0₂]² O rate=k[NO]²[0₂]³ O rate=k[NO]¹[0₂]³ [NO] (M) 0.0503 0.0247 Photo 0.0503 [0₂] (M) 0.0202 0.0202 0.0609 Rate (M/s) 0.355 0.0888 1.07 Done (+)