a) A series of experiments were caried out to determine the rate law for the following reaction: M+N+P Products The results are shown in the TABLE 1. Experiment [M] (mol L) N] (mol L) [P] (mol L) Rate (mol L's) 1 2y 2x 2y 3 2x 4y 4t 2x 4y 2z St TABLE 1 i What is the order of the reaction with respect to the concentration of M. N and P? ii. Write the rate law of the reaction i What is the unit of the rate constant?

a) A series of experiments were caried out to determine the rate law for the following reaction: M+N+P Products The results are shown in the TABLE 1. Experiment [M] (mol L) N] (mol L) [P] (mol L) Rate (mol L's) 1 2y 2x 2y 3 2x 4y 4t 2x 4y 2z St TABLE 1 i What is the order of the reaction with respect to the concentration of M. N and P? ii. Write the rate law of the reaction i What is the unit of the rate constant?

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 rate equation for a reaction between substances M and N is : rate = K[M]2 [N]2 The initial rate is found to be 7.5 × 10–3 mol dm-3 s-1 when the initial concentration of M is of 0.25 mol dm-3 and the initial concentration of N is 0.50 mol dm-3. Determine the value of k. Select one: O a. 0.24 s-1 O b. 0.12 s-1 O c. 0.96 s-1 d. 0.48 s-1
One typical reaction occurring in car engines is NO2+ CO (g)--------> NO (g) + CO2 (g) In order to determine the order of the reaction and the rate constant k, a series of three experiments were performed. The results are shown in the table Experiment Initial [NO2] (mol/L) Initial [CO] (mol/L) initial rate (v) 0.0050 0.080 0.0050 0.10 0.40 0.10 0.10 0.10 0.20 1 2 3 1-Write down the general expression for the rate of this reaction 2- Find the order for each reactant and the overall order for this reaction. Show your work ( 3- Find the value for k. Show your work 4- Based on these data, do you think that this is an elementary step or not? Briefly explain (
The following mechanism has been suggested for a reaction: NO(g) + Br2(g) → NOBR2(g) fast NOBR2(g) + NO(g) 2 NOBr(g) slow (a) What is the overall reaction? (b) What are the intermediates in the mechanism? (c) What is the rate law for the reaction? Edit View Insert Format Tools Table 12pt v Paragraph B IUA IMG F4 F5 F6 E10
A) In the proposed reaction mechanism below, the intermediate product is: A). NO(g) B). N2O2(g) C). H2(g) D). N2O(g) B) The rate expression for a particular reaction is rate = k[A][B]^2. If the initial concentration of B is increased from 0.10M to 0.30M, the initial rate will increase by which of the following factors A) 2 B) 3 C) 6 D) 9
Be sure to answer all parts. Rep Consider the reaction A+B Products From the following data obtained at a certain temperature, determine the order of the reaction. Enter the order with respect to A, the order with respect to B, and the overall reaction order. [A] (M) [B] (M) Rate (M/s) 1.50 1.50 3.20 x 10 1.50 2.50 3.20 x 10 Reaction 3.00 1.50 6.40 x 10 Proctorio is shaning your screen. Stop sharing
O KINETICS AND EQUILIBRIUM = 3/5 Using first- and second-order integrated rate laws Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. rate = (1.3 M¹-s¯¹) [₂0₁] olo Suppose a vessel contains N₂O5 at a concentration of 1.20M. Calculate the concentration of N₂O5 in the vessel 7.30 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M X Explanation Check Chelsea V @ EH
A certain reaction is second order in N, and second order in H,. Use this information to complete the table below. Be sure each of your answer entries has the correct number of significant digits. [N] [4] Initial rate of reaction 2.41 M 0.733 M 19.0 M/s 0.501 M 0.733 M Mls 0.873 M 2.02 M Mls dlo Ar
A reaction is identified as zero-order in one of its reactants, X. Time (s) [X] (M) 0 1.50 110 0.80 Based on the data and integrated rate law, what is the rate constant for the reaction at this temperature? k = [?] x 10 M-s-1 coefficient (green) exponent (yellow) Enter
Ⓒ Macmillan Learning Enter these data into the graphing tool and determine the value and units of the rate constant, k, for this reaction. Graphing Tool Add Row 10 total rows [A] [A] vs. t In[A] In[A] vs. t t (min) 0.0 2.0 4.0 6.0 1/[A] vs. t [A] (M) 1.00 0.66 0.43 0.28 1/[A] Clear All Data
8. Consider the reaction below: 2NO2 (9) (0ONZ Intial concentration of Initial concentration of O2 (mol/dm') Initial rate of formation of NO2 NO (mol/dm) (mol/dm) 0.12 0.05 0.12 0.12 0.10 0.24 0.24 0.05 0.48 Calculate the following The order of the reaction with respect to NO? The order of the reaction with respect to 02? i. ii. ii. The overall order of the reaction. iv. State clearly the units for this overall order reaction above in (ii) Calculate the value of the rate constant, k. V.
21. Platinum metal is used as a catalyst in the decompostion of NO(e) Into N,(g) and O,(g). A graph of the rate of the reaction as a function of NO concentration is shown below. (NOJ Explain why the rate stops increasing and levels out. Rate
g.