Determine the rate law and the value of k for the following reaction using the data provided.S20g 2 (aq) + 3 l'(aq) → 2 SO4 2 (g) + l3 (aq)[S2Og 2 l; (M) [1]; (M) | Initial Rate (M's')0.300.424.540.440.426.650.440.213.33Rate = 36 M's1 [S2O8 2 I]Rate = 23 M1/2s1 [S20g 2 JI]/2%3D2Rate = 120 M2s1Rate = 195 Ms1 [S2O8 2 PIT?Rate = 86 M2s1 [S20g 2 ?

Answer - The correct option is (A) Solution - According to the question - Given - Rate= k [S2O8-2]x…

Determine the rate law and the value of k for the following reaction using the data provided. S2Og ² (aq) + 3 l'(aq) → 2 SO4 ² (g) + l3 °(aq) [S20g 2 l; (M) [1]; (M) | Initial Rate (M's1) 0.30 0.42 4.54 0.44 0.42 6.65 0.44 0.21 3.33

Determine the rate law and the value of k for the following reaction using the data provided. S2Og ² (aq) + 3 l'(aq) → 2 SO4 ² (g) + l3 °(aq) [S20g 2 l; (M) [1]; (M) | Initial Rate (M's1) 0.30 0.42 4.54 0.44 0.42 6.65 0.44 0.21 3.33

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

For the reaction A + B C + D, various initial rate measurements were run beginning with A and B only, and beginning with C and D only. From the data below, calculate the rate law for both the forward and backward reactions. Then determine the equilibrium constant for the reaction. Rate (M/s) 1.081 x 10 6.577 x 10 6.568 x 10 [A] 0.660 [B] 1.23 4.01 1.23 2.25 4.01 Rate (M/s) 7.805 x 10 1.290 x 10" 1.300 x 10 [C] 2.88 [D] 0.995 2.88 1.01 1.65 1.65
12) At 25 °C, a certain elementary reaction has a forward rate constant equal 1.0 x 10-³ s' and an equilibrium constant, equal to 4.19. What is the rate constant for the reverse reaction?
The gas-phase decomposition of NOBr has a k= 0.82 M¹ s1 at 10°C. NOBr(g) → NO(g) + ½ Br₂ (g) rate k[ NOBr]² We start with 0.074 M NOBr in a flask at 10°C. 17T A. How long (in secs) does it take to use up 0.011 M of this NOBr? Only enter the number with no units 2.4
The rate constant for the reactionBr(g)+O3(g) --> BrO(g)+O2(g)was determined at the four temperatures shown in the table below. T (K) k [cm3/(molecule•s) 238 5.90 x 10-13 258 7.70 x 10-13 278 9.60 x 10-13 298 1.20 x 10-12 Plot the above data, and then use that data to calculate the activation energy for this reaction.
Nitrogen dioxide is a highly reactive gas! Determine the rate law and the value of k for the following reaction using the data provided: NO,(g) + O,(g) – NO,(g) + 0,(g) (w) P'ONI [0,1 (M) Initial Rate (M' s) 0.10 0.10 0.25 0.33 0.66 1.42 2.84 7.10 0.66 O Rate = 227 M25SINO,10j5 O Rate = 130 M2 s'[NO,10.J O Rate = 430 M2 s 'INO,ř10.] O Rate = 1380 M2.5 5INO, 10,1 O Rate = 43 M SINO,1O,]
Organic compounds that contain large proportions of nitrogen and oxygen tend to be unstable and are easily decomposed. Hexanitroethane, C2(NO2)6, decomposes according to the equation C2(NO2)6- 2NO, + 4NO + 2CO, The reaction in CCl, solvent is first order with respect to Cz{NO2)s At 63.7°C, k= 0.000254 s* and at 112.6°C, k = 0.0126s*. (a) What is the half-life of C2{NO2); at 63.7 °C? i seconds e Textbook and Media (b) What is the half-life of C2(NO2)s at 112.6 °C? seconds (c) IF0.100 mol of C2(NO2)6 is dissolved in CCI4 at 63.7°C to give 1.00 L of solution, what will be the C2(NO2), concentration after 50.0 minutes? i M (d) What is the value of the activation energy of this reaction, expressed in kilojoules? i kJ/mol (e) What is the rate constant at 159.4 °C?
Organic compounds that contain large proportions of nitrogen and oxygen tend to be unstable and are easily decomposed. Hexanitroethane, C₂(NO2)6, decomposes according to the equation C₂(NO2)6→ 2NO2 + 4NO+2CO2 The reaction in CCl4 solvent is first order with respect to C₂(NO₂)6. At 73.8 °C, k = 0.000330 s¹ and at 103.0 °C, k=0.0189 s ¹. (a) What is the half-life of C₂(NO2)6 at 73.8 °C? i eTextbook and Media (b) What is the half-life of C₂(NO₂)6 at 103.0 °C? i seconds (c) If 0.100 mol of C₂(NO2)6 is dissolved in CCl4 at 73.8°C to give 1.00 L of solution, what will be the C₂(NO2)6 concentration after 50.0 minutes? i M (e) What is the rate constant at 154.8 °C? i seconds (d) What is the value of the activation energy of this reaction, expressed in kilojoules? kJ/mol 51
Determine the rate law and the value of k for the following reaction using the data provided. NO,(9) + O3(g) – NO3(g) + O2(g) [NO,li (M) 0.1 0.1 [03li (M) Initial Rate (ms-1) 1 0.33 1.42 2 0.66 2.84 0.25 0.66 7.10 Rate = 43 M's INO,0,] S. -25c O Rate = 1360 M2s"INO,110,] S. Rate = 227 M25s INO,J[0,125 O Rate = 430 M?s INO,10,
2A(g) + 3/2B(g) Experiment e b) D d) k= 12345 Initial rate (mol/L.s) →→ C(g) 0.25*10-4 2.25x10-4 0.50×10-4 1.00×10-4 0.75*10-4 Initial [A] (mol/L) 5x10-2 15x10-2 5x10-2 10×10-2 5x10-2 unit: Overall reaction order is Rate = K[A][B] Initial [B] (mol/L) Reaction order with respect to A is Reaction order with respect to B is 5x10-2 5x10-2 10x10-2 5x10-2 15x10-2 O " O Calculate rate constant (k) based on data from experiment 3:
Consider the following elementary reaction: H,(9) +2NO(g) → N,0(g) +H,O(g) Suppose we let k, stand for the rate constant of this reaction, and k_, stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of H,O in terms of k, k_1, and the equilibrium concentrations of H, NO, and N,O. [H,0]= 0 %3D
The reaction CH;Br(aq) + OH (aq) - CH3OH(aq) + Br (aq) is first order with respect to each reactant. At a certain temperature, when the concentration of CH3Br is 0.565 M and the
State the types of each catalyst whether it's homogeneous catalysis heterogeneous catalysis or Biocatalysis 1. fetts ɔ. febrs 4. Fe(OTF)2 5. FelCI O4)2 · x H2O 6. Pda. 7 PdCl2 CM CN)2 8. Pd cacac)2 9 Pd Clz (PPh3), 10. Pd COA c)z [1. NaHSOy H20 9 Nalsor Ho 12. CH 3 SO3 H 13. AI(NOs) 9 H20 14. H3 040 PW12. XH2O 15. Fe: (S04)3 •9 HzO 16 Sn Cly• 5H2 O