Question 4KineticsThe formation of manganese oxide is an important consideration for many industrial processes, includingthe purification of ground water. The rate of formation, however, depends on the presence of variousinert gases, M:Mn2+ (s) + 0z(g) + M(g) # MnO2(s) + M(g)A petrochemical plant wants to improve their filtration procedures by using nitrogen as an inert gas (M =N2). Their research laboratory conducted the following kinetic experiments, involving different initialconcentrations of manganese and various mixtures of nitrogen and oxygen gas:[Mn'],(mol dm³)[N2].(mol dm')RateExperiment(mol dm³)1.25 x 102(mol dm³ min')2.63 X 10°11.0032.51.002.50 x 10232.51.05 X 10*31.001.25 x 10232.55.25 X 10°4.0.5001.25 x 10224.41.31 X 10°1.001.25 x 10216.32.63 X 10°Write down the rate law, indicating the order of each reactant concentration with respect to the reactionrate. (Show all your working and reasoning)4.14.2Calculate the reaction rate constant k, including units.

We have to determine rate law of given reaction and then find out its rate constant

Answered: Write down the rate law, indicating the…

Write down the rate law, indicating the order of each reactant concentration with respect to the reaction rate. (Show all your working and reasoning) 4.1 atant k including units.

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

The rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion present. The rate of decomposition was measured at constant temperature and pressure for various concentrations of H2O2 and of Kl. The data appear below. Determine the rate constant using the data from the first experiment. Rate (L min) [H2O2] [KI] ... 0.090 0.15 0.033 0.178 0.30 0.033 0.184 0.15 0.066 Round your answer to 2 decimal places.
For runs #1-#3 , calculate the rates of reaction. The reaction rate is : rate= 1/2 x molarity of sodium thiosulfate pentahydrate/ reaction time in seconds Indicate the units for each reaction rate. I know the the times are a little hard to read so here they are : run #1:117 seconds , run #2: 79.8 seconds ,run #3 :64 seconds.
1) Write the rate law given the following experimental results. Calculate the rate constant with the correct units.
The rate of a certain reaction is given by the following rate law: rate -k [N;][H,]* Use this information to answer the questions below. What is the reaction order in Ny? ? What is the reaction order in Hy? 2 What is overall reaction order? At a certain concentration of N, and Hy, the initial rate of reaction is 71.0 M/s. What would the initial rate of the reaction be if the concentration of Ny were doubled? Round your answer to 3 significant digits. M 17.8 The rate of the reaction is measured to be 0.290 M/s when (N)- 1.6 M and [H) - 0.71 M. Calculate the value of the rate constant. Round your answer to 2 significant digits.
7. The reaction (Tindak balas): 2HO2 (g)→ H2O2 (g) + O2 (g) With regard to HO2, calculate the reaction order and the rate constant k based on the following data: (Dengan merujuk kepada HO2, hitung tertib tindak balas dan pemalar kadar k berdasarkan data berikut:) Initial concentration [HO2] (M) (Kepekatan awal) 1.1 x 10-8 Experiment Initial Rate (M/s) (Eksperimen) (Kadar awal) 1.7 x 10-7 1 2 2.5 x 10-8 8.8 x 10-7 3.4 x 10-8 1.6 x 10-6 4 5.0 х 10-8 3.5 x 10-6
b. On the same diagram, draw a dashed line to indicate the changes that result from the addition of the catalyst. Explain the role of the catalyst in changing the rate of the reaction. 11. Given the following initial rate data: каза гази Rate (mole/Los) 1,350 12 TI T2 13,500 T3 54,000 a. What is the rate expression for the reaction? b. What is the value for k and its units? [A] .20 .50 .50 [B] .30 .60 1.2 c. What would happen to the rate if both the concentrations of A and B were doubled? 12. Consider a reaction of the form 2A + BC. The data for this reaction is given below: Initial rate of formation of C M/s Initial [A] Initial [B]
Last two parts please
A student follows the Determining the Rate Law for the Crystal Violet-Hydroxide lon Reaction procedure. The stock concentration of sodium hydroxide used in trial 1 is 0.021 M. The stock concentration of sodium hydroxide used in trial 2 is 0.010 M. Given the data below, what is the hydroxide ion concentration (M) in the trial 1 reaction mixture? Give your answer to four decimal places. Volume NaOH Volume Crystal Violet (mL) (mL) Trial 1 5.00 5.00 Trial 2 5.00 5.00
Some measurements of the initial rate of a certain reaction are given in the table below. Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol.
A. Why does catalyst is the factor that has the greatest impact on the rate of reaction in "exhaust from a car engine passes through a catalytic converter changing most of the poisonous nitrogen oxides into nitrogen gas and oxygen gas?" B. Why does concentration is the factor that has the greatest impact on the rate of reaction in "more bubbles appear when a concentrated solution of hydrochloric acid is added to a magnesium strip than when a dilute solution of the acid is added?"
Units of M s-1 please
Consider the following balanced chemical equation: H₂O2 (aq) + 31 (aq) + 2 H* (aq) → 13¯ (aq) + 2 H₂O (1) In the first 49.9 seconds of the reaction, the concentration of 13 increased from 0.692 M to 0.93 M. What is the average reaction rate over this time interval (in mol L-¹ s-¹)? Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". Answer: