G01222ad39. The catalysed reaction betweensulphur dioxide and oxygen is adynamic equilibrium: *2SO:(g) + O2(g) = 2SO3(g)AH=-196 kJ mol-Effect on the position ofequilibriumEffect on the rate of thereactionIncreasing the temperatureYWhich of the following is correct?YNo changeShifts to the leftShifts to the rightShifts to the leftA. No changeIncreasesB.C. IncreasesDecreases8324 umms6.16.235. Sucrose decomposes in acidicchange5.15.2solution into glucose and fructose16nent ofaccording to a first-order rate law,4.1rowthcurve 4.3 Ga+terns 3.3 M4.1 Dwith a half-Ilife of 3.33 h at 25 °C.What fraction of a sample of sucroseremains after 9.00 h? *AuctionPlantductive0.0134honesB.)0.154C. 0.561egnant18 Frnutation 3D. 0.814

Given that, change in enthalpy of the reaction ∆H = -196 kJ/mole The negative sign depicts that the…

35. Sucrose decomposes in acidic solution into glucose and fructose according to a first-order rate law, with a half-life of 3.33 h at 25 °C. What fraction of a sample of sucrose remains after 9.00 h? * A. 0.0134 B.0.154 C. 0.561 D. 0.814

35. Sucrose decomposes in acidic solution into glucose and fructose according to a first-order rate law, with a half-life of 3.33 h at 25 °C. What fraction of a sample of sucrose remains after 9.00 h? * A. 0.0134 B.0.154 C. 0.561 D. 0.814

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 following data regarding the concentration of a reactant during a single experiment was collected. What is the rate constant? a. 0.232 (mg/ml) / min b. 6.21 (mg/ml) / min c. 42.3 (mg/ml) / min d. 0.232 min-1 e. 6.21 min-1 f. 42.3 min-1
38. Time and concentration data were collected for the reaction A → B. t (s) [A] (M) 0.600 30.0 0.484 60.0 0.405 90.0 0.349 a. Determine the reaction order with respect to A. b. Calculate the rate constant for the reaction. 0.00
At 330 degrees Celsius, the rate constant for the second order decomposition of NO2 is 0.775M ^ - 1 * s ^ - 1 the Initial concentration of NO2 is 0.0500M a. Write the rate law expression for this reaction b. What is the concentration of NO2 after 30.0 minutes? c. How long in minutes will it take the concentration to decrease to 0.0050M? d. What is the half life for this reaction? e. What effect would doubling the NO2 concentration have on the rate of the reaction?
4. The decomposition of SO₂Cl₂ is first order in SO₂Cl₂ and has a rate constant of 1.42 x 104 s-¹ at a certain temperature. a. What is the half-life for this reaction? b. How long will it take for the concentration of SO₂Cl₂ to decrease to 25% of its initial concentration? c. If the initial concentration of SO₂Cl₂ is 1.00 M, how long will it take for the concentration to decrease to 0.78 M? d. If the initial concentration of SO₂Cl₂ is 0.150 M, what is the concentration of SO₂Cl₂ after 2.00 x 10² s?
5. A laboratory experiment was done for the reaction below and the following data was obtained: A→ Products a. Reaction order. Time (hours) Concentration of A, mg/L 0 1 Plot the data in Excel and determine the following: b. Reaction rate, k. 23468 135 119 104 88 73 41 10
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 KI. The data appear below. Determine the rate constant using the data from the first experiment.
8) A first order reaction starts with a concentration of reactant equal to 0.040 M. After two hours, the molarity is 0.020M. What is the molarity after four hours? a. 0.015M c. 0.005M e.0.03 М b. 0.010 M d.0.0025 M
d. There is too little information to assess the change. 8. If a reaction is first order with respect to [A], doubling the concentration of [A] will: a. double the rate of the reaction. b. increase the rate of the reaction fourfold. c. increase the rate of the reaction eightfold. d. not affect the rate of the reaction. 207 9. If a reaction is zero order with respect to [C], tripling the concentration of [C] will: a. triple the rate of the reaction. b. result in a fourfold increase in the rate of the reaction. c. result in a ninefold increase in the rate of the reaction. d. no impact on the rate of the reaction. 10. If a reaction is second order with respect to [B], doubling the concentration of [B] will: a. double the rate of the reaction. b. result in a fourfold increase in the rate of the reaction. c. result in an eightfold increase in the rate of the reaction. d. not affect the rate of the reaction. 11. For a second-order reaction, the plot of 1/[concentration] with respect to time…
37
The following data was obtained in a chemical kinetics experiment in which the concentration was measured every 10s. Determine the average rate of formation of product during the period from 20s to 70s.
Radioactive decay of 212Bi is observed to be a first-order process with a half-life (t½) of 4.00 days. It is noted that a 1.70 g sample of 212Bi decays over 12 days to leave only 0.213 g behind. What is the rate constant (k) for this process? a. 12.0 day–1 b. 0.250 day–1 c. 0.173 day–1 d. 5.77 day–1 e. none of these
The decomposition of NO2 is a second order reaction and the rate constant is 0.755 L/mol-s. In an experiment, the initial concentration of NO2 was 0.00650 mol/L. What is the half-life? Select one: a. 103.45 sec b. 304.56 sec c. 303.76 d. 203.76