The decomposition of N2O5 to NO2 and O2 is first order, with a rate constant of 4.80 x 10-4/s at 45°C. If the initial concentration of N2O5 is 7.85×10-2 mol/L,what is the concentration of N205 after 553 s?How long would it take for the concentration of N205 to decrease to 1.00 x 10-2 mol/L from an initial concentration of 7.85x10-2 mol/L?mol/L

Calculate final concentration and time....

The decomposition of N2O5 to NO2 and O2 is first order, with a rate constant of 4.80 x 10-4/s at 45°C. If the initial concentration of N205 is 7.85x10-2 mol/ what is the concentration of N205 after 553 s? How long would it take for the concentration of N205 to decrease to 1.00 x 10-2 mol/L from an initial concentration of 7.85x10-2 mol/L? mol/L

The decomposition of N2O5 to NO2 and O2 is first order, with a rate constant of 4.80 x 10-4/s at 45°C. If the initial concentration of N205 is 7.85x10-2 mol/ what is the concentration of N205 after 553 s? How long would it take for the concentration of N205 to decrease to 1.00 x 10-2 mol/L from an initial concentration of 7.85x10-2 mol/L? mol/L

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

For the zero-order decomposition of ammonia on tungsten NH3(g)-->1/2N2(g)+3/2H2(g) the rate constant is 2.08 x 10^-4 mol/L x s. How long will it take for the concentration of ammonia to drop from 1.44 M to 0.244 M, in hours?
The decomposition of N205 to NO2 and O2 is first order, with a rate constant of 4.80 x 10-4/s at 45°C. If the initial concentration of N2O5 is 4.85x10-2 mol/L, what is the concentration of N205 after 460 s? How long would it take for the concentration of N205 to decrease to 1.00 x 10-2 mol/L from an initial concentration of 4.85×10-2 mol/L? mol/L S
Consider the first-order decomposition of H2O2 with the rate constant of 1.8×10−5s−1 at 20 ∘C. How many hours will it take for the concentration to drop to 25%% of its initial value?
The decomposition of N2O5 to NO2 and O2 is first order, with a rate constant of 4.8e-4 1/s at 45°C. Let the inital concentration of N2O5 be 1.65e-2 mol/L. What is the half-life of the reaction? How long would it take for N2O5 to decrease to 1.00e-2 mol/L from its initial value? How long would it take for N2O5 to decrease to 75% of its inital value. Sketch [N2O5] versus time
A certain first order reaction has k = 2.51 s-1 . If the initial concentration of the reactant is 6.50 M, how much will be left after two half lives (in M)? Give your answer to three sig figs
The decomposition of N2O5 to NO2 and O2 is first order, with a rate constant of 4.80 × 10-4/s at 45°C. If the initial concentration of N2O5 is 7.98×10-2 mol/L, what is the concentration of N2O5 after 503 s? How long would it take for the concentration of N2O5 to decrease to 1.00 × 10-2 mol/L from an initial concentration of 7.98×10-2 mol/L?
The experimental rate law for the decomposition of nitrous oxide (N2O) and O2 is Rate = k[N2O]2. Which of the following could be a correct mechanism, explain why.
The decomposition of N2O5 to NO2 and O2 is first order with respect to the reactant N₂05 and first order overall. The rate constant for the reaction at 70.°C is 6.82x10-3 s-1. The reaction is started with 0.300 mol of N205 in a 0.500L container. What will the concentration of N2O5 be after 1.50 minutes? O a. 0.594M O b. 0.438M O c. 0.297M O d. 0.325M O e. 0.162M O f. 0.253M
The decomposition of nitrous oxide at 565 °C N₂O(g) → N₂ (9)+½O₂(g) 1 is second order in N₂O with a rate constant of 1.10 × 10-³ M s If the initial concentration of N₂O is 2.16 M, the concentration of N₂O will be M after 1480 seconds have passed.
1. You are going to do the boiling point experiment in the venting hood. Would you expect the observed boiling point of your positive control be exactly the true value? Why or why not?
Iodine atoms will combine to form I2 in liquid hexane solvent with a rate constant of 1.5×1010L/mol⋅s. The reaction is second order in I . Since the reaction occurs so quickly, the only way to study the reaction is to create iodine atoms almost instantaneously, usually by photochemical decomposition of I2. Suppose a flash of light creates an initial [I] concentration of 1.00×10−2 M How long will it take for 97% of the newly created iodine atoms to recombine to form I2? Express your answer using two significant figures.
The decomposition of hydrogen iodide on a gold surface at 150 °C HI(g) → ½ H2 (g) + ½ I2 (g) is zero order in HI with a rate constant of 1.20×10-4 M/s How much time is required for the concentration of HI to drop to 9.40×10-2 M if its initial concentration is 0.525 M?