Nitrogen dioxide undergoes thermal decomposition according to the second-order reaction 210,0→2NO+0₂ When 0.5000 MNO₂ is allowed to react for 9.00 minutes, its concentration falls to 0.0250 M. How long did it take for the concentration of NO₂ to fall to 0.2500 M a) 0.474 minute Ob) 4.74 minutes c) 0.592 minute d) 4.22 minutes Oe) 2.08 minutes

Nitrogen dioxide undergoes thermal decomposition according to the second-order reaction 210,0→2NO+0₂ When 0.5000 MNO₂ is allowed to react for 9.00 minutes, its concentration falls to 0.0250 M. How long did it take for the concentration of NO₂ to fall to 0.2500 M a) 0.474 minute Ob) 4.74 minutes c) 0.592 minute d) 4.22 minutes Oe) 2.08 minutes

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

How long will it take for the reaction to be 85% complete if it takes 32.0 min for the concentration of a reactant in a first-order reaction to drop from 0.55 M to 0.42 M at 298 K?
The decomposition of N2O5 is a first order reaction. 2N2O5 (g) 4NO2 (g) + O2(g) The rate of this decomposition is studied by monitoring the concentration of the reactant as a function of time, and the data obtained are shown in the following table: time (s) [N2O5] (M) 0.91 300 0.75 600 0.64 1200 0.44 3000 0.16 a) Plot In[N2O5] vs time using Excel (attach your plot picture) b) Determine the rate constant for this reaction. ||
Experimental data for the reaction A + 2B → C have been plotted in the following three different ways. 0.05 -3.0 0.04 0.03 0.02 0.01 0 IvI 0 2 Time (s) 1/[A] 100 80 40 20 0 In[A] -3.5 -4.0 -4.5 -5.0 0 2 Time (s) 2 Time (s) What is the order of the reaction, and what was the initial concentration of A? O first-order, initial concentration = 10 M second-order, initial concentration = 10 M zero-order, initial concentration = 10 M O second-order, initial concentration = 0.1 M O first-order, initial concentration = 0.1 M
The reaction A → B + C is found to be zero order. If it takes 4.2 102 seconds for an initial concentration of A to go from 0.58 M to 0.29 M, what is the rate constant for the reaction?
I need help with both of the blank spaces with correct significant figures
1. The following data were obtained for the reaction 3 A → 2 B: Time, s [A], M 10 15 20 0.200 0.0282 0.0156 0.0106 0.008 Determine the order of the reaction and rate constant.
The first-order rate constant for the decomposition of N2O5, 2N2O5 (g)→4NO2(g) + O2 (g) Part A at 70° C is 6.82 × 10¬3 s. Suppose we start with 2.60x10-2 mol of N2O5 (g) in a volume of 2.5 L. How many moles of N2O5 will remain after 4.0 min ? Express the amount in moles to two significant digits.
If the initial reactant concentration of a first order reaction is 1.60 M , what would be the concentration after 27 seconds ? Half-life = 9 s. 0.80 M 0.10 M 0.40 M 0.20 M
A gas mixture was prepared at 561 K with total pressure 3.27 atm and a mole fraction of 2.63x10 of HI and 3.54x10 of CH3. The elementary reaction HI(g) + CH3(g) I(g) + CH,(g) has a second-order rate constant of 3.50x10' L mol s at this temperature. Calculate the initial rate of the reaction under these conditions. mol L's Submit Answer 5 question attempts remaining
A chemical reaction of the general type: A → 2B is first-order, with a rate constant of 1.52 × 10-4 s-1. a) Calculate the half-life of A. b) Assuming the initial concentration of A is 0.067 mol L-1, calculate the time needed for the concentration to fall to 0.010 mol L-1.
The thermal decomposition of phosphine into phosphorus and hydrogen is a first order reaction with a half-life of 35.0 s at 680 °C. 4 PH3 (g) → P4 (g) + 6 H2 (g) a) Write the rate law for this reaction. b) How much time (in minutes) is required for 97% of a phosphine sample to decompose at 680 °C? c) If the activation barrier is 3.05 x 105 J/mol, what is the half-life for this reaction at 710 °C?
Dinitrogen pentoxide decomposes in the gas phase to form nitrogen dioxide and oxygen gas. The reaction is first order in dinitrogen pentoxide and has a half-life of 2.72 h at 25 °C. Part A If a 1.8 L reaction vessel initially contains 770 Torr of N2O5 at 25 °C, what partial pressure of O2 will be present in the vessel after 205 minutes? Express your answer in torr as an integer. P = VG ΑΣΦ ? Torr