For the overall chemical reaction shown below, which one of the following statements can be rightly assumed?2H2S(g) + O2(g) – 25(6) – 2H2O()Multiple ChoiceThe reaction is second-order overall.The rate law is, rete - KH,5? (02)The reaction is third-order overall.The rate law is, rate - KH2S)[O2).The rate law cannot be determined from the information given.

We have to predict the correct option for given transformation.

For the overall chemical reaction shown below, which one of the following statements can be rightly assumed? 2H2S(g) + O2(g) – 2s(s) ► 2H2O() Mulioie Choice The reaction is second-order overal. O The rate law is, rate - K+25?102) The reaction is third-order overall. a rate - KH25][O2l. The rate low is The rate law cannot be determined from the information given.

For the overall chemical reaction shown below, which one of the following statements can be rightly assumed? 2H2S(g) + O2(g) – 2s(s) ► 2H2O() Mulioie Choice The reaction is second-order overal. O The rate law is, rate - K+25?102) The reaction is third-order overall. a rate - KH25][O2l. The rate low is The rate law cannot be determined from the information given.

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

Consider this reaction: 2H,PO, (ag) – P,0, (aq)+ 3H,0 (aq) At a certain temperature it obeys this rate law. rate = (0.392 M-1.s Suppose a vessel contains H, PO, at a concentration of 0.520 M. Calculate how long it takes for the concentration of H, PO, to decrease to 12.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.
The decomposition reaction of ammonia gas (NH3) into hydrogen gas (H2) and nitrogen (N2) with a Pt catalyst is a zero order reaction at a temperature of 1130 K (i) rate of reaction = rate constant,(ii) reaction rate depends on ammonia concentration,(iii) the rate of decomposition of ammonia becomes constant when the ammonia has completely reacted,(iv) an increase in gas pressure will change the rate of the reaction. A. (ii) and (iv)B. (i) and (ii)C. (i), (ii) and (iii)D. (ii), (iii) and (iv)E. (i), (iii) and (iv)
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
3. Consider the reaction below: 2NO (g) + Cl,(g)'n 2NOCI (g) A mechanism involving these steps has been proposed for the reaction: Step 1: NO (g) + Cl,(g)'n NOCI, (g) Step 2: NOCI, (g) + NO(g)'n 2NOCI (g) The rate law for the reaction is given by rate = k[NO][Cl]. (a) What is the reaction intermediate? (b) Which is the rate-determining step? (c) Is the rate-determining step unimolecular, bimolecular, or termolecular? Why?
Consider the hypothetical reaction A(g) + B(g) C(g) The four containers below represent this reaction being run with different initial amounts of A and B. Assume that the volume of each container is 1.0L. The reaction is second order with respect to A and first order in respect to B. Which of the containers, W,X,Y or Z, would have the greatest reaction rate? Justify your answer.
A certain reaction has the following rate law: rate = k[X]³[Y]² Which of the following are the correct units for k? Select one: L³mol-3s-1 Ms-1 M³s O L?mol2s1 L5mol 5s1 Lmol-'s mol³L-3s-1 M's-1 L*mol-4s-1 mol?L-2s1
Consider the reaction described by the equation C,H,Br, (aq) + 3 I (aq) C,H, (g) + 2 Br¯(aq) + I5 (aq) The rate law is rate = k[C,H¸Br,][I¯] where k = 0.00504 M-1. s-1. What are the missing entries in the table? Run [C,H,Br,h (M). [I¯], (M) Initial rate of formation of C,H, (M-s) 1 0.162 0.000529 0.162 y 0.000265 3 0.162 0.162 M X = M y = z = M-s-1
2 YO2 (g) + X2 (g) → 2 YO₂X (g) = -218 kJ/mol reaction AH rxn The reaction is first-order with respect to YO2 and first-order with respect to X₂. What is the relationship between the rate constant and activation energy of a chemical reaction?|
Consider the reaction described by the equation С,Н, Вr, (aq) + 3Г (аq) — С,н,(8) + 2 Br (aq) + I5 (aq) The rate law is rate = k[C,H,Br,][I¯] where k = 0.00594 M-1. s-!. What are the missing entries in the table? Run [C,H,Br, lo (M) [I-], (M) Initial rate of formation of C,H, (M-s -) 1 0.245 0.00143 0.245 y 0.000713 3 0.245 0.245
Ln [A] Post Lab Assignment 1. Nitrosyl chloride, NOCI, decomposes to NO and Cl2. 2NOCI(g) → 2NO(g) + Cl, (g) Determine the rate law, the rate constant, and the overall order for this reaction from the following data: [NOCI] (M) Rate (mol L-1 h-1) 0.10 0.20 0.30 3.2 x 10-9 7.2 x 10-9 2. A 5.0 mL dye solution of 3.45 e-5 M is mixed with 15.0 mL bleach solution of 0.21 M. What are the initial concentrations of [Dye] and [Bleach] for your experiment? 3. The plots of 1/[A] vs time, In([A]) vs. time, and [A] vs. time of a solution of substance A are shown below. What is the reaction order with respect to A? 000 009 007 000 0 20 40 Time (min) Time 09 08 Time
Consider this reaction: 2C1,0, g) → 2C1, (6) + 50, (g) At a certain temperature it obeys this rate law. rate = (0.36 Ms)[C1,0,1 %3D Suppose a vessel contains Cl,0, at a concentration of 0.630 M. Calculate how long it takes for the concentration of Cl,0, to decrease to 5.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.
The reaction is 2A3 3B2 + F The corresponding rate law is, rate = k[A3]² [F]. It means that the overall order %3! is... second order first order zero order third order