For the following reaction, use the plots below to determine the reaction order withrespect to NO₂ (g):Reaction: 2NO₂ (g) → 2NO(g) + O₂ (g)[NO2] vs Time0.0100.0080.006y = -1.017E-05x + 6.942E-03R² = 0.89540.0040.0020.000200300400500Time (s)In[NO2] vs Time-4.5-5.0y = -2.250E-03x -4.933R² = 0.9737-5.5-6.0-6.5300400500Time (s)[NO2]In[NO2]0100100200600600 1/[NO2]5004003002001001001/[NO2] vs Time200y = 5.408E-01x + 1.250E+02R² = 1.000300400500Time (s)600

Given : We have to tell the order of NO2 .

For the following reaction, use the plots below to determine the reaction order wit respect to NO2 (8): Reaction: 2NO2 (g) → 2NO(g) + O₂ (8) [NO2] vs Time 0.010 0.008 y = -1.017E-05x + 6.942E-03 0.006 R² = 0.8954 0.004 [NO2]

For the following reaction, use the plots below to determine the reaction order wit respect to NO2 (8): Reaction: 2NO2 (g) → 2NO(g) + O₂ (8) [NO2] vs Time 0.010 0.008 y = -1.017E-05x + 6.942E-03 0.006 R² = 0.8954 0.004 [NO2]

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 general rate law for the reaction is given by rate = k[NH4+]x[NO2-]y. Determine the order with respect to each reactant (i.e. solve for x and y). X = Y = Then determine the value of the rate constant, k (provide your answer to two significant figures). Rate constant, k = x 10 --
The rate constant for the reaction 2N2O5(g) → 4NO2(g) + O2(g) is equal to 3.41 x 10–5 s–1 at 30 ºC. If the initial concentration of N2O5is 0.446 M what concentration of NO2 will be observed after 175 minutes? Assume that initially no NO2 was present in the reaction vessel.
A reaction has a rate constant of k = 2.55 s¹. What is the overall reaction order? Equations: Rate = K[A][B]² kı[A2] = k-1[A]² -Ea In[A] = -akt + In[A]o k = Ae RT In 2 Ea t₁/2 = Ink In A- ak RT 1 1 Ea/1 = 2kt + [A] = [A]o In (*) - (-+) RT₁ T₂ 1 t1/2 2k[A]o O1st order 2nd order 3rd order 4th order O None of the above.
The reaction CH3-N=C – → CH3-C=N is a first-order reaction. At 230.3 °C, k= 6.29 x 10–4s-1. If [CH3-N=C] is 1.00 × 10-3 initially, [CH3-N=C]is M after 1.000 x 103 s.
The reaction described by the equation O₂(g) + NO(g) →→→ O₂(g) + NO₂(g) has, at 310 K, the rate law rate: rate of reaction = -4 Given that [03] = 8.0 × 10−4 M and [NO] = 3.0 × 10-5 M at t = 0, calculate the rate of the reaction at t = 0. k[O3 ][NO] k = 3.0 × 106 M-¹.s-¹ What is the overall order of this reaction? O 0 2 3 1 M/S
A reaction has a rate constant, k = 0.0866 M-1 s-1. What is the half-life (seconds) when the initial concentration is 4.27 M?
1
The reaction rate for the decomposition of N2O5 to form NO2 and O2 was studied as a function of temperature. The first order reaction rate constants were found to be: T(K) k(s-1) 273 7.9 x10-7 298 3.5 x10-5 308 1.4x10-4 318 5.0x10-4 328 1.5x10-3 338 4.9x10-3 What is the Ea for this reaction in kJ/mol? Use Excel to plot the pertinent data and use linear regression to calculate the slope of the line connecting your data.
The reaction I (ag) + OCI (ag) → IO (ag) + Cl¯(aq) was studied, and the following data were obtained: I]o (mol/L) [OCI¯], (mol/L) Initial Rate (mol/L · s) 0.080 0.14 7.90 x 10-2 0.040 0.14 4.00 x 10–2 0.020 0.070 9.90 × 10–3 -2 0.16 0.070 7.90 x 10 What is the rate law? (Use k for the rate constant.) Rate = Calculate the value of the rate constant. k = L/mol · s Calculate the initial rate for an experiment where both I and OCI are initially present at 0.14 mol/L. Rate = mol/L · s
mm
The tabulated data shows the concentration of N2O5 versus time for the reaction: N2O5=NO3+NO2 Time, s [N2O5], M 0 1.0 25 .822 50 .677 75 .557 100 .458 125 .377 150 .310 175 .255 200 .210 Determine the order of the reaction.
Data in the table were collected at 540 K for the following reaction: CO + NO2 = CO2 + NO Determine the reaction order with respect to each reactant. Order with respect to CO: Order with respect to NO2