FontParagraphWe are determining the rate law equation for a reaction A+ B +C ABC in which a dramatic andinstant color change tells us that reactants are used up and product is formed. (Concentrations used inall experiments are [A] = 2.0M, [B] = 1.0M and [C] = 3.0M)This is the data for questions 11 through 14:Volume of water,Time from mixing to dramatic colorchange, secVolume ofVolume ofVolume ofА,В,C,mlmlmlml0.52.02.095.5361.02.02.095.011) Which reactant concentration have we changed?a) Аb) вc) сd) no reactant concentrations changed12) What was the change in concentration of that reactant?a) no changeb) doubledc) tripledd) increased by the power of 1013) What was the change in reaction time?a) no changeb) slower time = (faster time) x 2c) slower time = (faster time) to the power of 2d) there is no relationship between reaction times and concentration changege 5 of 7* Accessibility: Investigate99+e Type here to searchASUSF4F2三F1F3Esc34.5.18

Time for completion of reaction in first trial = 36 s = (6) 2 s Time for completion of reaction in…

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) %3D %3D This is the data for questions 11 through 14: Time from mixing to dramatic color change, sec Volume of Volume of Volume of Volume of water, A, B, C, ml mL ml ml 0.5 2.0 2.0 95.5 36 1.0 2.0 2.0 95.0 6. 11) Which reactant concentration have we changed? a) A b) в c) C d) no reactant concentrations changed 12) What was the change in concentration of that reactant? a) no change b) doubled c) tripled d) increased by the power of 10 13) What was the change in reaction time? a) no change b) slower time = (faster time) x 2 c) slower time = (faster time) to the power of 2 d) there is no relationship between reaction times and concentration change %3D 1412 words * Accessibility: Investigate

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) %3D %3D This is the data for questions 11 through 14: Time from mixing to dramatic color change, sec Volume of Volume of Volume of Volume of water, A, B, C, ml mL ml ml 0.5 2.0 2.0 95.5 36 1.0 2.0 2.0 95.0 6. 11) Which reactant concentration have we changed? a) A b) в c) C d) no reactant concentrations changed 12) What was the change in concentration of that reactant? a) no change b) doubled c) tripled d) increased by the power of 10 13) What was the change in reaction time? a) no change b) slower time = (faster time) x 2 c) slower time = (faster time) to the power of 2 d) there is no relationship between reaction times and concentration change %3D 1412 words * Accessibility: Investigate

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

Consider the generic reaction below. A + B --> C + D Given the following data and graph, determine the rate law for the reaction. Trial 1 [A] 0.10 M [B] 0.10 M Absorbance (A 1.55- 1.50 1.45- 1.40- 0 Trail 2 0.14 M 0.10 M 0.5 Trial 1 - Trial 2 1.0 Time (s) Trial 3 0.10 M 0.20 M Trial 3 1.5 2.0
Ab 22
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
A1.
Consider the reaction: H2 (g) +I2 (g) → 2 HI (g) A chemist performed an experiment and monitored the concentration of I2 during the course of the reaction. The red line in the graph below represents the results obtained. Which line in the plot would best represent how the concentration of HI changes during the course of the reaction? Time (s) Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a a b b d d е е Concentration (M)
True or False (6 - 7) 6. It is found for the reaction A + B → C that doubling A while keeping B constant makes the reaction go 8 times faster and doubling B while keeping A constant makes the reaction go 2 times faster. The rate law for this reaction is: rate= k (A][B]* 7. Suppose you were dissolving a metal such as zinc with hydrochloric acid. Particle size of zinc has no effect on the rate of reaction.
Answer all the questions in the image.
The starting concentration (time zero) of crystal violet is 1 x 10-4 M. Using the proper integrated rate law and the calculated value for k, calculate the concentration of crystal violet after 240 seconds. Look at the equation of the trend line for your lost linear graph and the beer-lambert law. Equation from graph from NaOH 0.0660M is y= -0.0105x-0.6277
3) A chemical reaction was conducted at 4 different temperatures and the following data was obtained. Plot the In(k) versus the inverse of the respective temperature using linear regression analysis (Excel). Find the slope (from the graph) and what does that number represent? Use Arrhenius equation. Calculate the Activation Energy for the reaction. Rate constant (k) Temperature of reaction (°C) 0.0521 15 0.101 25 0.184 35 0.332 45 NOTE: Make sure to attach the graph paper with proper calculation.
ew K History Bookmarks DZL Rate Laws Expe X Profiles Tab Determination c X 1 Homework 2 ttempt 1 Listen Window my.edu/d21/le/content/408344/viewContent/17004406/View Help Your Answer: Rates Law Expe X D21 4. CLASS SLIDE X 3 What is the rate constant for a reaction based on the following experimental information? Expt Rate (M/s) [A] (mol/L) [B] (mol/L) 1 0.5170 0.700 0.648 2 1.4912 1.189 0.648 1.2205 1.529 D21 Activity Assignr X 0.700 Report your answer to THREE significant figures. A ALEKS-Isabell x E
1. indicate the activation energy for the overall reaction on the graph. (You may want to use a line for the sake of clarity.)2. Write the elementary reactions that make up the reaction mechanism. 3. What would you propose as the rate law for this reaction? 4. Of course, this proposed law is hypothetical. Using the following data collected experimentally (probably using a UV/vis spectrometer J), determine the rate law for this reaction. Include reaction order and the value and units for k. Please show your work, including any graphs you make. (Note: no credit will be given to correct final answers without supporting work.) Does your experimental rate law match the one you proposed above?
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