Directions: Answer the following questions. Determine the rate law from the initial rates. 1. Determine the rate law and the rate constant for the reaction from the following experimental data: Acetaldehyde decomposes when heated to yield methane and carbon monoxide according to the equation: CH:CHO( CHagi+CO(a) [CH3CHO] Trial Initial Rate 1 1.75 x 103 2.06 x 101 2 3.50 x 103 8.24 x 10-11 7.00 x 103 3.30 x 1010

Directions: Answer the following questions. Determine the rate law from the initial rates. 1. Determine the rate law and the rate constant for the reaction from the following experimental data: Acetaldehyde decomposes when heated to yield methane and carbon monoxide according to the equation: CH:CHO( CHagi+CO(a) [CH3CHO] Trial Initial Rate 1 1.75 x 103 2.06 x 101 2 3.50 x 103 8.24 x 10-11 7.00 x 103 3.30 x 1010

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

Given reaction rate data for: H2O2 + 31" + 2H* → I3 ¯ + 2H2O Trial [H2O2] M [1'] M [H'] M Rate (M/s) 1.15 х 10 2.30 x 106 2.30 x 106 1.15 x 106 1 0.010 0.020 0.010 0.010 0.020 0.010 0.00050 0.00050 0.00050 0.00100 3 4 0.010 0.010 Write the rate law for the reaction. O a. Rate = k[H2O2][I¯ ][H¯ ] O b. Rate = k[H202]²[I¯ ][H¯ ] O c. Rate = k[H2O2]?[I" ] O d. Rate = k[H2O2][I¯ ]?[H¯ ] O e. Rate = k[H2O2][I¯ ]
Given the following results: Run Rate of Reaction (M/s) [I-] [H2O2] 1 1.99 0.516 0.561 2 3.15 0.516 0.643 3 5.22 0.817 0.561 Calculate the rate constant(k) for each run. Assuming the Rate Law = k[I-]2[H2O2] calculate the average rate constant,k, for this reaction. Give your answer to 2 places after the decimal.
19. The initial rate of decomposition of acetaldehyde at 600°C was measured at a series of concentrations with the following results. Solve for the rate law expression of this reaction. Note: Include all rough notes, show all calculations, follow the rules of significant figures, and box your final answer. ( CH;CHO(g) → CH,(g) + CO(g) Trial Number Trial #1 Trial #2 Trial #3 Trial #4 [CH,CHO] 0.10 M 0.20 M 0.30 M 0.40 M Initial rate 0.085 0.34 0.76 1.4 (mol/L-s)
1. Determine rate law expression, overall order of reaction and rate constant based on the data for the reaction A+B products. [A] [B] 1.50 1.50 1.50 2.50 3.00 1.50 Rate(M/s) 0.320 0.320 0.640
how do i solve this?
Solve the question at 398 k for the reaction rate data for the equation. Calculate the value of the rate constant at the given 398 k temperature value.
a) Acetone is a good solvent due to its ability to dissolve both polar and nonpolar substances, while other solvents can only dissolve one or the other. Pharmaceuticals, scientific testing, sterilizing medical tools, cosmetics, textiles, and gasoline, all require the use of acetone as a cleaner or solvent. At high temperature, acetone decomposes in a first order process to methane and ketene. At 600 °C, the rate constant is 8.7 x 103 s. i) What is the half-life of the reaction? ii) How long does it take for 40% of a sample acetone to decompose?
This is your graph. The rate of reaction at any point in time is given by the gradient of the concentration-time graph. Annotate your graph to show how you could determine the rate of reaction at 6 hours by drawing a tangent to the curve. Include your annotated graph in the answer and use the values from it to calculate the rate of reaction at 6 hours. Show your calculation in full.
8. The temperature dependence of the acid-catalyzed hydrolysis of penicillin is investigated, and the rate constant k is found to be 7.0x10+ s' at 22.2 °C and 2.5×10 s¹ at 38.0 °C. What is the activation energy of the hydrolysis reaction? a) 61.6 kJ/mol b) 54.4 kJ/mol c) 45.8 kJ/mol d) 50.7 kJ/mol calculate the solubility
Round any decimals to the nearest integer value.Use negative exponents instead of placing a concentration in the denominator of a fraction.Do not use multiplication symbols or spaces in the rate laws. 1. The rate doubles when [NO] is doubled and [Br2] remains constant. 2. The rate doubles when [Br2] is doubled and [NO] remains constant. 3. The rate increases by 1.56 times when [NO] is increased 1.25 times and [Br2] remains constant.
Rate Expressions: Write the rate expression and the rates of all other species using the given rate for the stated reactions. Make sure the reactions are balanced. 3. N₂ + O₂ → N₂0s N₂ + S0₂ → N₂ 205 Rate of depletion of O₂ = 0.79M/s 4. C₂H6+ O₂-3H₂O +2CO₂ Rate of formation of CO₂= 1.32M/s 5. H₂O2)→ H₂O(g) + O2(g) Rate of formation of H₂O = 1.21M/s
1a. According to the mechanism of bromination, what is the intermediate’s structure of the following reaction 1b. According to the mechanism, what is the intermediate’s structure of the following reaction