In a study of the decomposition of ammonia on a platinum surface at 856 °C NH31/2 N2 + 3/2 H, the following data were obtained: NH3), M seconds 3.90x10-3 1000 1.95×10-3 1.50x103 9.75x10-4 1.75x103 7.80×10-3 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 7.80×103 M i ( Mis [ Js and when the starting concentration is 3.90×10-3 (2) The average rate of disappearance of NH3 from t =0 s to t = 1000 s is| ]Ms'. (3) The average rate of disappearance of NH3 from t=1000 s to t = 1.50×10³ s is ]Ms!. (4) Based on these data, the rate constant for this [ ) order reaction is | Ms!.

In a study of the decomposition of ammonia on a platinum surface at 856 °C NH31/2 N2 + 3/2 H, the following data were obtained: NH3), M seconds 3.90x10-3 1000 1.95×10-3 1.50x103 9.75x10-4 1.75x103 7.80×10-3 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 7.80×103 M i ( Mis [ Js and when the starting concentration is 3.90×10-3 (2) The average rate of disappearance of NH3 from t =0 s to t = 1000 s is| ]Ms'. (3) The average rate of disappearance of NH3 from t=1000 s to t = 1.50×10³ s is ]Ms!. (4) Based on these data, the rate constant for this [ ) order reaction is | Ms!.

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

In a study of the gas phase decomposition of dinitrogen pentoxide at 335 K N₂O5(g) 2 NO₂(g) + 1/2O₂(g) the concentration of N₂O5 was followed as a function of time. It was found that a graph of In [N₂O5] versus time in seconds gave a straight line with a slope of -7.00x 10-3 s-¹ and a y-intercept of -1.96. Based on this plot, the reaction is order in N₂O5 and the rate constant for the reaction is
In a study of the gas phase decomposition of sulfuryl chloride at 600 KSO2Cl2(g)SO2(g) + Cl2(g)the concentration of SO2Cl2 was followed as a function of time.It was found that a graph of ln[SO2Cl2] versus time in minutes gave a straight line with a slope of -4.28×10-3 min-1 and a y-intercept of -6.95 . Based on this plot, the reaction is________. (firest, zero, or second) order in SO2Cl2 and the rate constant for the reaction is min-1.
Give a clear handwritten answer with explanation...?
The following data was obtained for the decomposition of X2 in the gas phase. X2→Y + Z 0.00 2.00 4.00 6.00 8.00 10.00 12.00 14.00 16.00 18.00 20.00 (hr) [X2] 0.250 0.213 0.182 0.155 0.133 0.113 0.097 | 0.082 0.070 0.060 0.051 a. Determine the rate constant for this reaction. b. How much X2 is left if 0.457 M of the gas is allowed to decompose for 1.75 hours? c. What is the half-life of 0.892 M X2?
Give good explanation Asap Thanks
cvg.cengagenow.com The following data are for the gas phase decomposition of dinitrogen pentoxide at 335 K. 2 NO₂(g) + 1/ 0₂(g) N₂05(g) - - [N₂O5 ], M time, s 0.199 0 S OWLV2 | Online teaching and learning resource from Cengage Learning 9.95x10-2 116 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is In progress (2) Based on these data, the rate constant for this 4.98x10-2 2.49x10-² 232 348 + 88 S. 99% order reaction is 2.
11:27 2NH4+ (aq) + HCO3- (aq) The reaction is first order with respect to urea, and first order overall with a rate constant of 4.28 x 10^(-4)s^(-1) a. Write the rate law for this reaction. b. If the reaction begins with an initial urea concentration of 0.500 M, what will the concentration of urea in the solution be after 2500 s? C) Calculate the half life of this reaction. d. At what time (+) will the concentration of urea be 0.020 M? O □
I need a solution within 15 minutes
In a study of the decomposition of ammonia on a platinum surface at 856 °C NH3¬1/2 N2 + 3/2 H, the following data were obtained: NH3), M 1.95x10-3 1.50x103 9.75x10-4 1.75x103 7.80×10-3 3.90x10-3 seconds 0 1000 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 7.80×103M is s and when the starting concentration is 3.90×103 Mis (2) The average rate of disappearance of NH3 from t= 0 s to t= 1000 s is ]Ms!. (3) The average rate of disappearance of NH3 from t= 1000 s to t= 1.50×103 s is ]Ms!. (4) Based on these data, the rate constant for this v order reaction is Ms!
kindly help me here? please, I'll rate you. thanks!
In a study of the gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g) 2 NO2(g) + ½ O2(g) the concentration of N,O5 was followed as a function of time. It was found that a graph of In[N½O5] versus time in seconds gave a straight line with a slope of -7.29×103 s and a y-intercept of -1.44. Based on this plot, the reaction is v order in N,Og and the rate constant for the reaction is Submit Answer Try Another Version 2 item attempts remaining
please answer!