### Chemical Kinetics: Rate Equations and Reaction Orders**7. Substances P and Q react together to form products and the overall order of the reaction is three. Which of the following rate equations could not be correct and why?**- **A**: rate = k \[P\]^2 \[Q\]- **B**: rate = k \[P\]^0 \[Q\]^3- **C**: rate = k \[P\] \[Q\]^2- **D**: rate = k \[P\] \[Q\]^3- **E**: rate = k \[P\] \[Q\]^2 \[H\]^0**8. The reaction between three reactants A, B, and C was studied. The initial rates of reaction at different concentrations of the three reactants were measured and are given in the following table:**| experiment | \[A\] / mol dm-3 | \[B\] / mol dm-3 | \[C\] / mol dm-3 | Initial rate / mol dm-3 s-1 ||--|--|--|--|--|| 1 | 1.0 | 1.0 | 1.0 | 2.3 × 10-3 || 2 | 1.0 | 3.0 | 1.0 | 6.9 × 10-3 || 3 | 2.0 | 3.0 | 1.0 | 1.4 × 10-2 || 4 | 2.0 | 1.0 | 2.0 | 4.6 × 10-3 |#### a) Deduce the partial orders of reaction with respect to A, B, and C.#### b) Calculate the value of the rate constant, giving its units.#### c) Write the rate equation.**Graph/Diagram Explanation:**The table provided in question 8 lists the concentrations of reactants A, B, and C in different experiments along with the initial rates of reaction. This data can

Rate equation may be defined as an equation that links the rate of forward reaction with the…

7. Substances P and Q react together to form products and the overall order of the reaction is three. Which of the following rate equations could not be correct and why? A rate = k [P]2 [Q] D rate = k [P][Q]³ E rate = K[P][Q]²[H*]° B rate= k [P] [Q]³ C rate = k [P] [Q]² 2.1, 2.2 L3 8. The reaction between three reactants A, B and C was studied. The initial rates of reaction at different concentrations of the three reactants were measured and are given in the following table: [A]/mol dm3 [B]/mol dm3 [C]/mol dm-3 1.0 3.0 3.0 1.0 experiment 1 2 a) b) c) 3 4 1.0 1.0 2.0 2.0 1.0 1.0 1.0 2.0 Deduce the partial orders of reaction with respect to A, B and C. Calculate the value of the rate constant, giving its units. Write the rate equation. Initial rate/mol dm³ s-1 2.3x10-3 6.9×10-3 1.4×10-² 4.6×10-3 21.2.2L3

7. Substances P and Q react together to form products and the overall order of the reaction is three. Which of the following rate equations could not be correct and why? A rate = k [P]2 [Q] D rate = k [P][Q]³ E rate = K[P][Q]²[H*]° B rate= k [P] [Q]³ C rate = k [P] [Q]² 2.1, 2.2 L3 8. The reaction between three reactants A, B and C was studied. The initial rates of reaction at different concentrations of the three reactants were measured and are given in the following table: [A]/mol dm3 [B]/mol dm3 [C]/mol dm-3 1.0 3.0 3.0 1.0 experiment 1 2 a) b) c) 3 4 1.0 1.0 2.0 2.0 1.0 1.0 1.0 2.0 Deduce the partial orders of reaction with respect to A, B and C. Calculate the value of the rate constant, giving its units. Write the rate equation. Initial rate/mol dm³ s-1 2.3x10-3 6.9×10-3 1.4×10-² 4.6×10-3 21.2.2L3

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 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)
Consider the following reaction: + NH4" (aq) + NO2 (aq) → N2(g) + 2H2O(I) The rate law is given by the following equation. Rate = k [NH4"][NO2"] a. At a certain temperature, the rate constant is 2.80 × 10 -4 /M•s. Calculate the rate of the reaction at that temperature when [NH4"]= 0.26M and [NO2]=0.23M b. From the above information, state the overall order of the reaction. 89 c. State what effect on the rate of reaction you would expect to see if you increased the temperature in this experiment. Briefly explain your reasoning. |
The reaction of NOBr(g) to form NO(g) and Br2(g) is second order: 2NOBr(g) → 2NO(g) + Br₂(g) The rate constant is 0.556 L mol-¹ s¹ at some temperature. If the initial concentration of NOBr in the container is 0.21 M, how long will it take for the concentration to decrease to 0.028 M? t = S
Ozone reacts with nitrogen dioxide to produce oxygen and dinitrogen pentoxide according to the following chemical equation: O3(g) + 2NO2(g)→ 02(g) + N2O5(g) The rate law for this reaction is Rate = k[O3]|NO2]. If concentration is measured in moles per liter and time is measured in seconds, what are the units of k?
1 2 3 4 5 8 7 A chemical engineer is studying the rate of this reaction. NH OH(aq) →NH, (aq)+H,O(aq) He fills a reaction vessel with NH OH and measures its concentration as the reaction proceeds. Here's a graph of his data: t (s) Use this graph to answer the following questions: 발 pe here to search (W) [HO'HN] 6 H hp Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | 80°F Partly s