22. For the reaction2 NO(g) + 2 H;(g)N3(g) + 2 H;O(g)at 1100 "C, the following data have been obtained:Initial [Ha] (M)0.320.320.64Rate of Na (M/s)0.0120.0240.048ExperimentInitial [NO] (M)5.0 x101.0 x1025.0 x103Determine the initial rate of N;(g) production for a mixture of 0.25 M NO(g) and0.50 M H2.47 M/sb. 0.017 M/s0.22 M/sd. 2800 M/s1.5 M/s3.с.c.

Answered: Image /qna-images/answer/21d8ffd3-8de4-4cfa-a2b8-a0ccf26aef3c.jpg

22. For the reaction 2 NO(g) + 2 H3(g) → N;(g) + 2 H;O(g) at 1100 "C, the following data have been obtained: Rate of Na (M/s) 0.012 0.024 0.048 Experiment Initial (Hal (M) Initial (NO) (M) 5.0 x10 1.0 x10 5.0 x10 0.32 0.32 0.64 2 3. Determine the initial rate of N;(g) production for a mixture of 0.25 M NO(g) and 0.50 M H2. 47 M/s b. 0.017 M/s 0.22 M/s d. 2800 M/s a. c.

22. For the reaction 2 NO(g) + 2 H3(g) → N;(g) + 2 H;O(g) at 1100 "C, the following data have been obtained: Rate of Na (M/s) 0.012 0.024 0.048 Experiment Initial (Hal (M) Initial (NO) (M) 5.0 x10 1.0 x10 5.0 x10 0.32 0.32 0.64 2 3. Determine the initial rate of N;(g) production for a mixture of 0.25 M NO(g) and 0.50 M H2. 47 M/s b. 0.017 M/s 0.22 M/s d. 2800 M/s a. c.

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

a) A chemical reaction is given below. Write the rate of the reaction with respect to each reactant and product. CH3 + 50, → 3Co, + 4H,0 b) A Kinetic experiment gives the following data for the following reaction. Find the average rate of the reaction between t=0 sec to t=15 sec and also between t= 5 sec and t-20 sec. OCr +r → Ol + Cr [ OCr ]M 1.2 0.8 0.3 0.6 0.4 t (sec) 0 5 10 15 20
Determine the average rate of change of B from t :0 s to Time (s) Concentration of A (M) t = 252 s. 0.740 126 0.425 A → 2B 252 0.110 rateB = M/s
ess important values if needed for this question. For the decomposition of hydrogen lodide on a gold surface at 150 °C 2 HI(g) → H₂(g)+ 12 (9) the average rate of disappearance of HI over the time period from t=0s to t=2610s is found to be 1.20 x 10 M-s¹. The average rate of formation of I₂ over the same time period is M-s Submit Answer Retry Entire Group 9 more group attempts remaining
The reaction 2 N205(g) → 4 NO2(g) + O2(g) was studied and the rate of change of the concentration of O2 was found to be 3.65 mol L 15-1. Calculate the reaction rate (in mol L1s1). Reaction rate = i mol L-1s-1. eTextbook and Media Save for Later Attempts: 0 of 3 used Submit Answer
7
5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T
Use the data presented in the table to determine the rate equation for the hypothetical reaction shown. A(g) + 2B(g) + 3C(g) [Math Processing Error] D(g) + 2F(g) Exp {A} (M) {B} (M) {C} (M) initial rate (M/min) 0.0025 0.0025 0.0025 3.16x10-11 0.0025 0.0050 0.0025 1.27x10-10 3 0.0050 0.0050 0.0025 1.27x10-10 4 0.0100 0.0100 0.0050 4.06x10-9 What is the reaction order with respect to A? What is the reaction order with respect to B? What is the reaction order with respect to C? Enter each of your answers numerically as integers or fractions (ex: 0, 1/2, 1, 3/2, 2, 3, etc). Hint: Determining the order of one of the reactants will be difficult. Determine the order of the two easy reactants first, then use that information in determining the difficult one.
Which of the following is true for the rate law r= k[A]M[B]"? O A) The order of each species must be determined by experiment. B) Both m and n are restricted to positive integers. C) Both m and n can be obtained from the stoichiometry of the overall reaction. D) The overall order of the reaction is given by m x n.
Q2) Calculate the rate constant for the first order decomposition reaction of phosphine [PH3], M (at 120 °C): 4PH3(g)→ P4(g) + 6H₂(g)? .64 * 10 ^ - 2 Time (sec) a) 2.47 * 10 ^ - 2 * s ^ - 1 0 2.32 *10^ - 8 1.16 * 10 ^ - 2 (5.80 * 10 ^ - 3)/84 b) 28s ^ - 1 c) 4.64*10^ -2 overline s^ -1 56 d) 3.57 * 10 ^ - 2 * s ^ - 1
Fe3+ (aq) + 7.00 SCN- (aq) → Fe(SCN)7.00 3+ (aq) 1.)Find the rate where SCN- is consumed, if Fe3+ is consumed at 1.00 M/min. 2.) Find the rate and the overall order of the rate law
O https://app.101edu.co A * Question 7 of 20 Determine the rate law for the reaction A+ B - C + D given the following experiment data. Initial Trial [A]o [B]o Rate A) Rate = k[A] %3D (M/min) B) Rate = k[A]? 1 0.25 0.40 7.25 C) Rate = k[A][B] %3D 2 0.75 0.40 21.5 D) Rate = k[A]°[B] %3D 3 0.50 0.80 14.5 E) Rate = k[A][B] 4 0.75 0.80 21.5 Delete F12 wwwn D F11 FI0 FO FB FS FO Backspace Num Lock F2 %3D 1 8. 6. 4 12 3 Wome E R Enter J K F S. Shift Poyblip Ctr Alt Home All
Fill in the 2 question marks on the table given the data