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 5 through 8: Volume of Volume of Volume of Volume of water, mL Time from mixing to dramatic color change, sec A, B, C, mL mL mL 0.5 2.0 2.0 95.5 36 1.0 2.0 2.0 95.0 6

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 5 through 8: Volume of Volume of Volume of Volume of water, mL Time from mixing to dramatic color change, sec A, B, C, mL mL mL 0.5 2.0 2.0 95.5 36 1.0 2.0 2.0 95.0 6

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

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!
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,=11.0 kJ/mol. If the rate constant of this a 1 - 1 reaction is 3.2 × 10° M S. at 112.0 °C, what will the rate constant be at 149.0 °C? Round your answer to 2 significant digits. 1 - 1 k = ] M x10 •S ?
- 1 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0020 M·s 2 HI (g) → H, (g) + I, (g) Suppose a 4.0 L flask is charged under these conditions with 150. mmol of hydrogen iodide. How much is left 5.0 s later? 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.
Chemistry When entering compound units, indicate multiplication of units explicitly using a multiplication dot For example, M^−1⋅s^−1 M^−1⋅s^−1. Express your answer to two significant figures and include the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot or a dash.
A chemistry graduate student is studying the rate of this reaction: NH4OH(aq)—>NH3(aq)+H2O(aq) He fills a reaction vessel with NH4OH and measures its concentration as the reaction proceeds (shown in picture). A. Write the rate law for this reaction B. Calculate the value of the rate constant k. Round your answer to two significant digits. Also be sure your answer has the correct unit symbol.
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)
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
Consider the reaction: A - → 2C The concentration of reactant A and product B were monitored at the same time interval. Time t, Minutes Molar Concentration A, [A] Molar Concentration C, [C] 0 2.40 0.00 2.00 2.20 0.40 4.00 2.00 0.80 1. Calculate the change in the concentration of A per unit time (M/min) from time (t=0 min) to time (t=2.00 min). Mark the box with an X to identify your choice of the correct answer. (5 pts) + 0.20 M/min + 0.10 M/min - 0.20 M/min - 0.10 M/min
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
The Reaction below should be used for questions 4 and 5. IO3 − + 5I− + 6H+ → 3I2 + 3H2O The oxidation of iodide ions by iodate ions in acidic aqueous solution occurs according to the stoichiometry shown above. The experimentally determined rate law of the reaction is rate = k[IO3 − ] [I− ] According to the rate law for the reaction, an increase and decrease in the concentration of hydrogen ion has what effect on this reaction?