Kinetic data at relatively short times for the reactionCo(g) + NO 2(g) → CO 2(g) + NO(g)at 120 °C are given in the table below:Experiment[CO] (mol L-1)INO21 (mol L-1)Initial rate (mol L-1 h-1)5.0 x 10-45.0 x 10-4|1.0 × 10-3|0.36 x 10-40.18 x 10-40.36 x 10-43.4 x 10-81.7 x 10-86.8 x 10-8Which on of the following expressions is the rate law for the reaction at short times in the specified conditions.A. rate = k [CO] [NO2)· rate = k [CO]-1 [NO2)-1* rate = k [CO]-1/2 [NO2]· rate = k [CO] [NO2]2rate = k [CO] [NO2]1/2

Given in the question, The complete balanced equation, CO (g)+ NO2 (g) →CO2 (g) + NO (g) Let, rate =…

Kinetic data at relatively short times for the reaction Colg) + NO 2(g) → CO 2(9) + NO(g) at 120 °C are given in the table below: Experiment cO] (mol L-1) 10-4 NO2) (mol L-1) b.36 х 10-4 Initial rate (mol L-1h-1) 5.0 x 34 х 10-8 1.7 × 10-8 6.8 x 10-8 5.0 x 10-4 0.18 x 10-4 1.0 × 10-3 6.36 x 10-4 Which on of the following expressions is the rate law for the reaction at short times in the specified conditions. O A. rate = k [CO] [NO2] * rate = k (CO]r1 [NO21"1 C. rate = k (CO]"1/2 (NO2] O D. rate = k [CO] [NO2]2 %3D OE. rate = k [CO] [NO2]1/2

Kinetic data at relatively short times for the reaction Colg) + NO 2(g) → CO 2(9) + NO(g) at 120 °C are given in the table below: Experiment cO] (mol L-1) 10-4 NO2) (mol L-1) b.36 х 10-4 Initial rate (mol L-1h-1) 5.0 x 34 х 10-8 1.7 × 10-8 6.8 x 10-8 5.0 x 10-4 0.18 x 10-4 1.0 × 10-3 6.36 x 10-4 Which on of the following expressions is the rate law for the reaction at short times in the specified conditions. O A. rate = k [CO] [NO2] * rate = k (CO]r1 [NO21"1 C. rate = k (CO]"1/2 (NO2] O D. rate = k [CO] [NO2]2 %3D OE. rate = k [CO] [NO2]1/2

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...

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4. The following data were obtained for the follwing chemical reaction: 2A+38->2C+D Trial # Initial (A) Initial [B] Initial Rate of Formation (mmol/L) (mmol/L) of D (mmol/L."s) 1 4.0 6.0 1.60 2 2.0 6.0 0.80 3 4.0 3.0 0.40 (a) Determine the rate law equation for this reaction. Show your reasoning. (T: 2) (b) Find the rate constant, k, with units. (T: 2)
Can my answers be checked please thank you .
Write rate law for the chemical reaction ?
4. The following data were obtained for the follwing chemical reaction: 2A + 3B ---> 2C + D Initial [A] Initial [B] Initial Rate of Formation Trial # (mmol/L) (mmol/L) of D (mmol/L*s) 1 4.0 6.0 1.60 2 2.0 6.0 0.80 3 4.0 3.0 0.40 (a) Determine the rate law equation for this reaction. Show your reasoning. (b) Find the rate constant, k, with units.
For the hypothetical reaction A + 2B 3C, the rate of appearance of C given by (A[C]/At) may also be expressed as O A[C]/At = -(2/3) A[B]/At O A[C]/At = -(3/2) A[B]/At O A[C]/At = -(1/2) A[A]/At %3D O A[C]/At = A[A]/At
A reaction is described as follows: k1 X + Y The table below shown the initial rates of the formation of product Z (Vo) for various reactant concentrations. From the data given, answer the followings: [X], mol L- [Y], mol L-1 34 Vo (x 103 mol L-s') 22 1.00 70 45 4.20 8.08 71 89 (i) The rate law of formation of product Z, (ii) The overall rate order and the order with respect to each component, and (iii) The rate constant (state clearly its units and coefficients).
2. Consider the reaction A+2B C whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: [v] (M) (M) (M/s) [B] Rate Trial 1 0.10 0.050 6.0x10-4 0.10 0.100 1.2x10-3 3 0.20 0.050 2.4x10-3 Part B Provide
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Consider this initial rate data at a certain temperature in the table for the reaction Determine the rate law. OCI (aq) + (aq)- k= rate = k OH(aq) [OCIT] [OH] →OI (aq) + Cl(aq) [1] [1-1² Answer Bank [OH-]² Trial 1 2 3 4 [OCIT [I lo [OCI ]o (M) (M) 0.00179 0.00179 0.00179 0.00322 0.00281 0.00179 0.00179 0.00322 Determine the value of the rate constant for this reaction and the correct units. Units [OH Jo (M) 0.490 0.490 0.681 0.867 Initial rates (M/s) 0.000440 0.000792 0.000497 0.000448