Write the rate law for the decomposition of ammonium nitrite into nitrogen gas and water using the following data. NH4* (aq) + NO2 (aq) → N28) + 2H2O Trial (NH4*4]; (NO21]}; Rate (M/s) 1 0.010 0.20 5.4x10-7 0.020 0.20 10.8x10-7 0.20 0.020 10.8x10-7 4 0.20 0.040 21.6x107 2. 3.

Write the rate law for the decomposition of ammonium nitrite into nitrogen gas and water using the following data. NH4* (aq) + NO2 (aq) → N28) + 2H2O Trial (NH4*4]; (NO21]}; Rate (M/s) 1 0.010 0.20 5.4x10-7 0.020 0.20 10.8x10-7 0.20 0.020 10.8x10-7 4 0.20 0.040 21.6x107 2. 3.

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 2HI→ H₂+I2. The rate of disappearance of HI follows the second order rate law. A[HI] = -k[HI]² At The rate constant kis 2.01 x 10-2 M-1s-1. What was the initial concentration of HI (in units of molarity) if the concentration of HI was found to be 0.262 M after t = 45.0 s? Report your answer using three significant figures. Provide your answer below: M rate
For the gas phase decomposition of ethyl acetate, CH;COOC,H5–CH;COOH + C,H4 the rate constant in s1 has been determined at several temperatures. When In k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.41×10“ K and a y-intercept of 28.8. The value of the rate constant for the gas phase decomposition of ethyl s1. acetate at 675 K is (Enter your answer to one significant figure.)
Using the data in the table, determine the rate constant of Trial [A] (M) [B] (M) Rate (M/s) the reaction and select the appropriate units. 1 0.280 0.200 0.0163 A +2B C+ D 0.280 0.400 0.0163 0.560 0.200 0.0652 Units k =
Given the following results: Rate of Run Reaction [1] (M/s) 1.76 0.358 0.476 4.72 0.358 0.843 5.25 0.672 0.476 1 2 3 [H₂O2] Calculate the rate constant(k) for each run. Assuming the Rate Law = k[1]²[H₂O₂] calculate the average rate constant,k, for this reaction. Give your answer to 2 places after the decimal.
Q1
It may not surprise you to know that products can show up in the rate law. When the product(s) is(are) a positive order, we describe the rate law as autocatalytic. For example, under conditions of high nitric acid concentrations, this reaction: HNO, + H₂C(OH): → HNO; + HCOOH + H₂O has a rate law: rate = k [H.C(OH).] [HNO₂] Given a rate constant of 0.0255 dm3 mol-1 s-1 and initial concentrations [HNO,] = 5.0 mol dm-3, [H.C(OH).]. = 150 mmol dm-3, [HNO:]. = 8.2 mmol dm-3, how long will it take for the methanediol concentration to fall to 52 mmol dm-3?
A student suspects that the nitrate ion (NO3−), rather than the Cu2+ ion, is the active species in the Cu(NO3)2 catalyst. He devises a second experiment to test his hypothesis, using KNO3 as a potential catalyst. If the student's hypothesis is correct, what should he observe when KNO3 is added to the reaction? Any changes are observed relative to an identical un-catalyzed reaction. a. The rate of the reaction will decrease b. The rate of the reaction will increase c. There will be no change in the rate of the reaction
A student suspects that the nitrate ion (NO3−), rather than the Cu2+ ion, is the active species in the Cu(NO3)2 catalyst. He devises a second experiment to test his hypothesis, using KNO3 as a potential catalyst. If the student's hypothesis is incorrect, what should the student observe when he adds KNO3 to the reaction? Any changes are observed relative to an identical un-catalyzed reaction. a. The rate of the reaction will decrease b. The rate of the reaction will increase c. There will be no change in the rate of the reaction
Nitrogen dioxide is a highly reactive gas! Determine the rate law and the value of k for the following reaction using the data provided: NO,(g) + O,(g) – NO,(g) + 0,(g) (w) P'ONI [0,1 (M) Initial Rate (M' s) 0.10 0.10 0.25 0.33 0.66 1.42 2.84 7.10 0.66 O Rate = 227 M25SINO,10j5 O Rate = 130 M2 s'[NO,10.J O Rate = 430 M2 s 'INO,ř10.] O Rate = 1380 M2.5 5INO, 10,1 O Rate = 43 M SINO,1O,]
20.) A generic reaction has the rate law rate = k[A]2[B]0. What [A], in moles per liter, will be required to give a rate of = 0.383 M/s when the [B] = 0.181 M? The value of the rate constant is 0.344. Do not include units. Your Answer:
Consider the reaction below which can occur during the reforming process when manufacturing high octane gasoline: 3 C4H4 → 2 C6H6 or: 3 cylclobutadience → 2 benzene The average rate of appearance of benzene is given by Δ[benzene]/Δt. If we compare the rate of appearance of benzene and the rate of disappearance of cyclobutadiene, we get Δ[benzene]/Δt = ____________×(-Δ[cyclobutadiene]/Δt). What should be written in the blank? Question 1 options: A) -2/3 B) +2/3 C) -3/2 D) +1 E) +3/2
In aqueous solution, CIO reacts to produce CIO3 and CI", according to the following chemical equation. 3 CIÓ (ag) → CIO3¯ (ag) + 2 CI- (aq) A plot of 1/[CIO ] vs. time is linear, with a slope equal to 0.056 M-1s-1. If the initial concentration of CIO- is 0.56 M, how long will it take for half of the ClIO to react? 27 sec O 12 sec O 32 sec O 0.036 sec O 7.1 sec