Give typed full explanation not a single word hand written otherwise leave it The following data are for the decomposition of nitramide in aqueous solution at 25 °C. NH2NO2(aq) N2O(g) + H2O(l) [ NH2NO2 ], M 0.640 0.320 0.160 8.00×10-2 time, min 0 164 328 492 Hint: It is not necessary to graph these data. (1) The half-life observed for this reaction is ___ min .
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Give typed full explanation not a single word hand written otherwise leave it
The following data are for the decomposition of nitramide in aqueous solution at 25 °C.
NH2NO2(aq) N2O(g) + H2O(l)
| [ NH2NO2 ], M | 0.640 | 0.320 | 0.160 | 8.00×10-2 |
| time, min | 0 | 164 | 328 | 492 |
Hint: It is not necessary to graph these data.
(1)
The half-life observed for this reaction is ___ min .
(2)
Based on these data, the rate constant for this ___ order reaction is ___ min -1.
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- The decomposition of N,O, can be described by the equation 2N,0, (soln) –→ 4 NO, (soln) + 0, (g) Consider the data in the table for the reaction at 45 °C in carbon tetrachloride solution. 1 (s) [N,O;] (M) 2.287 165 2.062 466 1.706 725 1.449 Given the data, calculate the average rate of reaction for each successive time interval. What is the average rate of reaction for the time interval from 0 s to 165 s? average rate of reaction: 0.00136 M/s Incorrect What is the average rate of reaction for the time interval from 165 s to 466 s?In a study of the rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NH,NCO(aq)→(NH,),CO(aq) the following data were obtained: (NH,NCO], M 0.146 1.83x10 2 S.66x10 7.30x102 3.65x102 minutes 2.44x10 812 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.146 M is concentration is 7.30x102 M is min and when the starting min. (2) The average A(1/[NH,NCO]) / At from t= 0 min to t- 812 min is The average A(1/[NH,NCO]) / At from t= 812 min to t= 2.44x103 min is M1 min M' min . (3) Based on these data, the rate constant for this v order reaction is M1 min !In a study of the decomposition of ammonia on a platinum surface at 856 °C NH3-1/2 N₂ + 3/2 H₂ the following data were obtained: [NH3], M seconds 5.79x10-3 0 2.90x10-3 998 1.45x10-3 7.25x10-4 1.50x10³ 1.75x103 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 5.79x10-³ M is starting concentration is 2.90x10-³ M is S. (2) The average rate of disappearance of NH3 from t = 0 s to t = 998 s is (4) Based on these data, the rate constant for this (3) The average rate of disappearance of NH3 from t = 998 s to t = 1.50x10³ s is order reaction is M s ¹. M S-1 Ms¹. s and when the
- [References) Use the References to access important values if needed for this question. In a study of the gas phase decomposition of dimethyl ether at 500 °C CH;OCH;(g)- →CH4(g) + H2(g) + CO(g) the concentration of CH,OCH, was followed as a function of time. It was found that a graph of In[CH,OCH] versus time in seconds gave a straight line with a slope of -6.28x10s and a y-intercept of -3.50 Based on this plot, the reaction i Đ order in CH,OCH, and the rate constant for the reaction is zero first second Submit Answer Try Another Version 2 item attempts remaining (Previous 12 étv ll MacBook Air 80 DII DD F2 F3 F4 F5 F6 F7 F8 F9 F10 F11 @ #3 $ & * 4 6. 7 8 W E R Y { S G J K く C V ...- ~の * 00 ラ エ BIn 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 3.90x10-3 1000 1.95x10-3 1.50x103 9.75x10-4 1.75x103 7.80x10-3 seconds Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 7.80×10-3 M is| s and when the starting concentration is 3.90x103 M is (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 Ms!. order reaction is52-56. For the reaction 2N,O5(g) → 4NO,(g) + O2(g), the following data were collected: t (minutes) [N,O;] (mol/L) 1.24 x 10-2 10. 0.92 x 10-2 20. 0.68 x 10-2 30. 0.50 x 10-2 40. 0.37 x 10-2 50. 0.28 x 10-2 70. 0.15 x 10-2 52. The order of this reaction in N,O, is a) 0 b) c) 2 d) 3 1 none of these
- In an aqueous solution of 0.100 M of CH₂BrCOONa and 0.00801 M of S2O3Na2, the following interchange reaction takes place. CH₂BrCOO - (aq) + S₂O3²− (aq) - CH2S203C00 2- (aq) + Br(aq) At temperature of 25 ° C, the non-ideal observed rate constant for the reaction is 1.07 M-¹ s-¹. Assuming the following ionic strength equation is valid for this reaction in its aqueous solution, log10 knon-ideal estimate the values of the rate constant for zero ionic strength. = log10 kideal + 2A ZA ZB √I 1+√IAG° (kJ per mole O₂) -300 -600 -1050 4 Cu + O₂-2 Cu₂0 .…....... 2 Zn + 0₂ → 2 ZnO 2C+0₂-2 CO 4/3 AI + O₂ → 2/3 Al₂O, 1000 Temperature (°C) 2000 What is the overall reaction when 2Zn(s) + O2(g) → 2ZnO(s) +701kJ is coupled with the reduction of Cu₂0(s) to Cu(s)? Will it be spontaneous at 1000 Celsius? Why and why not?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)
- Consider the reaction: NO(g) + C₂H₂(g) → HCN(g) + CO(g) + H(g), is The Arrhenius expression for the reaction is k(T) = 8.97 x 10-¹2 cm³ molec-¹ s¹ exp{-218 kJ mol-¹/RT} over the temperature range 1100 - 1500 K. Using transition state theory, calculate AH* and AS* for this reaction at 1300 K.write the mechanism 2.3 NaOH, H₂O & Heat34. A key step in the formation of sulfuric acid from dissolved SO2 in acid precipitation is the oxidation of hydrogen sulfite ion by hydrogen peroxide: HSO, (ag) + H2 O2 (aq) → HSO, (aq) + H2O(t) The mechanism involves peroxymonosulfurous acid, SO20OH¯: k1 HSO, (aq) + H2 O2 (ag) 2 SO200H (ag) + H2 O (l) k-1 k2 SO200H (aq) + H3O+ (aq) → HSO, (ag) + H3O† (aq) By making a steady-state approximation for the reactive intermediate concentration, [SO20OH (ag)], express the rate of formation of HSO, (aq) in terms of the concentrations of HSO, (aq), H2O2 (aq), and H3 O“(aq).