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: 2.00×103 5.00x104 1.50x103 1.00x10-3 2.50x104 1.75x103 NH3), M seconds 998 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 2.00x10 3 M is s and when the starting concentration is 1.00x10 M is (2) The average rate of disappearance of NH3 from t =0s to t = 998 s is |Ms. (3) The average rate of disappearance of NH3 from t= 998 s to t=1.50x103 s is |Ms.

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: 2.00×103 5.00x104 1.50x103 1.00x10-3 2.50x104 1.75x103 NH3), M seconds 998 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 2.00x10 3 M is s and when the starting concentration is 1.00x10 M is (2) The average rate of disappearance of NH3 from t =0s to t = 998 s is |Ms. (3) The average rate of disappearance of NH3 from t= 998 s to t=1.50x103 s 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

Please solve all thrree parts , for any HELPful ratings from me.
In a study of the decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C N₂O5 2 NO2 + 12 0₂ the concentration of N₂O5 was followed as a function of time. It was found that a graph of In[N₂05] versus time in minutes gave a straight line with a slope of -5.74×10-³ min-¹ and a y-intercept of -1.78. Based on this plot, the reaction i zero first second order in N₂O5 and the rate constant for the reaction is min-¹.
The decomposition of dinitrogen pentoxide gas at 318.15K is measured as the decrease of N,O5 concentration in partial pressures (mm): The data are shown graphically: Time (s) [N2O5] (mm) 348 6 247 12 195 24 105 36 58 48 33 60 18 72 10 Calculate the rate constant for the reaction. Use Excel to plot the pertinent data and use linear regression to calculate the slope of the line connecting your data.
In a study of the gas phase decomposition of dinitrogen pentoxide at 335 KN2O5(g)2 NO2(g) + ½ O2(g)the concentration of N2O5 was followed as a function of time.It was found that a graph of ln[N2O5] versus time in seconds gave a straight line with a slope of -6.20×10-3 s-1 and a y-intercept of -2.02 .Based on this plot, the reaction is order in N2O5 and the rate constant for the reaction is s-1.
In a study of the gas phase decomposition of sulfuryl chloride at 600 K so,Cl,(g)SO2(g) + C½(g) the concentration of SO,Cl, was followed as a function of time. It was found that a graph of In[SO,Ch] versus time in minutes gave a straight line with a slope of -3.89×103 min and a y-intercept of -5.85. Based on this plot, the reaction is order in SO,Cl, and the rate constant for the reaction is min
For the decomposition of nitramide in aqueous solution at 25 °C NH,NO,(aq)N,0(g) + H,0(1) the following data have been obtained: NH,NO,], M 0.388 0.193 9.56x10-2 4.75x10-2 time, min 248 496 744 The average rate of disappearance of NH,NO, over the time period from t= 0 min to t= 248 min is M min.
Eyring equation in term of concentration can be written as ats atH kr where n = 1 or 2 Given: E = A+H + 2RT gas (bimolecular) Ea = A+H + RT solution, and gas (unimolecular) %3D Write an expression of A+S in terms of preexponential factor for the reaction 2NOCI (g) 2NO (g) + Clz (g)
In a study of the decomposition of ammonia on a tungsten surface at 1100 °CNH31/2 N2 + 3/2 H2the following data were obtained: [NH3], M 1.31×10-2 6.55×10-3 3.28×10-3 1.64×10-3 seconds 0 441 661 771 Hint: It is not necessary to graph these data. FILL IN THE BLANKS(1)The observed half life for this reaction when the starting concentration is 1.31×10-2 M is _______s and when the starting concentration is 6.55×10-3 M is _______s.(2)The average rate of disappearance of NH3 from t = 0 s to t = 441 s is ______ M s-1.(3)The average rate of disappearance of NH3 from t = 441 s to t = 661 s is _______M s-1.(4)Based on these data, the rate constant for this _______ (zerofirstsecond) order reaction is_______ M s-1.
A certain reaction has an activation energy of 66.0 kJ mol' and a frequency factor of A1 = 6.80x1012 L mol 's1. What is the rate constant, k, of this reaction at 22.0 °C? Express your answer with the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot (asterisk) or a dash. • View Available Hint(s) HẢ X•10" k = 5.277 L•mol-1 1 •S
Assuming the collision factor is the same for both situations, calculate the difference in activation energies for the uncatalyzed (Ea) versus the enzyme-catalyzed (Eac) reaction. Express your answer in kilojoules to two significant figures.
In a study of the rearrangement of cyclopropane to propene at 500 °C (CH2)3 CH3CH=CH2 the concentration of (CH2)3 was followed as a function of time. It was found that a graph of In[(CH2)3] versus time in seconds gave a straight line with a slope of -9.38×104 s1 and a y-intercept of -1.57 . Based on this plot, the reaction is O order in (CH2)3 and the half life for the first reaction is seconds.
In a study of the formation of HI from its elements,H₂(g)+I₂(g)→ 2HI(g) equal amounts of H₂ and I₂ were placed in a container, whichwas then sealed and heated.(a) On one set of axes, sketch concentration vs. time curves for H₂ and HI, and explain how Qchanges as a function of time.(b) Is the value of Qdifferent if [I₂] is plotted instead of [H₂]?