Given the following data for this reaction: A(g) + 2 B(g) ====> 2 C(g) Determine the differential rate law. Experiment [A], [B], Initial RATE 1 0.020 M 0.010 M 0.020 M/s 2 0.020 M 0.015 M 0.030 M/s 0.010 M 0.010 M 0.005 M/s Rate = k[A][B] Rate = k[A]2[B] Rate = k[A][B]2 Rate = k[A]2[B]2
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- Are the following processes examples of homogeneous or heterogeneous catalysis? a Hydrolysis of immiscible ethyl acetate (l) in an aqueous basic solution. b Conversion of NOX gases to N2 and O2 by platinum metal. c Decomposition of atmospheric ozone by NO gas. d Oxidation of ethyl alcohol, C2H5OH, by the enzyme alcohol dehydrogenase, ADH, to acetaldehyde in the body. e Solid-state conversion of C graphite to C diamond by transition metal additives at high pressure.List at least four experimentally determined parameters that you, an experimenter, can define when exploring the hydrolysis of ethyl benzoate by aqueous sodium hydroxide.Ne(g) effuses at a rate that is ______ times that of Kr(g) under the same conditions. rateNe/rateKr=
- [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 conversion of methyl isonitrile to acetonitrile in the gas phase at 250 °CCH3NC(g)CH3CN(g)the concentration of CH3NC was followed as a function of time.It was found that a graph of ln[CH3NC] versus time in seconds gave a straight line with a slope of -4.38×10-3 s-1 and a y-intercept of -2.83 . Based on this plot, the reaction is ______ order in CH3NC and the half life for the reaction is _______ seconds.2. Consider the kinetic data of the reaction of P + 2 Q + 2+ - PQ, + Z*and answer the succeeding questions: Experiment P (M) Q (M) Temp ("C) Initial Rate, M/s 1 0.01150 0.01200 0.00000 25 4.80 x 10-4 2 0.02300 0.01200 0.00000 25 1.92 x 10-3 3 0.01150 0.02400 0.00000 25 9.60 x 10-4 4 0.04600 0.01200 0.00000 25 7.68 x 10-3 5 0.01150 0.04800 0.00000 25 1.92 x 10-3 6 0.01150 0.01200 0.00000 10 5.10 x 10-5 0.01150 0.01200 0.00000 40 4.55 x 10-3 0.01150 0.01200 0.00500 10 4.98 x 10-5 0.01150 0.01200 0.01050 25 4.82 x 104 10 0.01150 0.01200 0.02100 40 4.44 x 10-3 A. Determine the rate order with respect to P. Determine the rate order with respect to Q. C. Determine the rate law of the reaction. What is the average rate constant? Indicate the appropriate units. E. What is the energy of activation and frequency factor of the reaction without the additive ion? Include the equation of the best fit line of the Arrhenius equation and RSQ Note: Use the calculated rate constant in set up 1 for 25°C…
- Nitric oxide reacts with hydrogen to release large amounts of chemiluminescence with the characteristics of the highly cytotoxic species. The following data were measured for the reaction of nitric oxide with hydrogen: Data number 1 2 3 2 NO(g) + 2 H₂(g) → N₂(g) + 2 H₂O(g) [NO] (M) 0.1 0.1 0.2 [H₂] (M) 0.1 0.2 0.1 Based on the data, (a) Determine the rate law for this reaction. (b) Calculate the rate constant. (c) Calculate the rate when [NO] = 0.050 M and [H₂] = 0.150 M Initial rate (M/S) 1.23 x 10-³ 2.46 x 10-³ 4.92 x 10-³Determine the average rate of change of B from t = 0 s to Time (s) Concentration of A (M) t = 352 s. 0.760 176 0.450 A → 2 B 352 0.140 rateg = M/s TOOLS x10 NOV étv 1 MacBook Air 80 888 DII DD F12 F3 F9 F10 F11 F4 F5 F6 F7 F8if the rate at which O2 appears change [O2]/change t=6.0 x 10-5 Mol s-1 at a partivular instant at what rate is O3, disappearing at the same time - change[O3 ]/change in time
- Determine the average rate of change of B from t = 0 s to Time (s) Concentration of A (M) t = 352 s. 0.760 176 0.450 A 2 B 352 0.140 rateB = M/s - TOOLS x10 NOV 1 étv MacBook Air 80 DII DD F4 F5 F6 F7 F8 F9 F10 F11 F12 %23 & *(a) The decomposition of a gas phase reactant, A, into gaseous products, P and Q, proceeds according to the reaction stoichiometry: A (g) P (g) + Q (g) and has been studied by measurement of the pressure increase in a constant volume system. Starting with an initial pressure of 112 torr of pure A at 713 K, the following total pressures, were measured at the times stated: Time (min) Pressure (Torr) | 136 15 30 45 60 75 155 170 181 191 (i) Give a suitable expression for the integrated rate equation by which the tabulated data can be analysed to confirm that the reaction exhibits first order kinetics. (ii) Calculate the rate constant and the half life of the reaction. (ii) If the activation energy of the reaction is given by 120 kJ mol, determine the rate constant and half life at a temperature of 1100 K.In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g)V½ H2(g) + ½ I½(g) the concentration of HI was followed as a function of time. It was found that a graph of 1/[HI] versus time in seconds gave a straight line with a slope of 1.72×103 M1s1and a y-intercept of 0.667 M1. Based on this plot, the reaction is order in HI and the rate constant for the reaction is M1s1