3. The gas phase decomposition of N2O5 was studied at a constant temperature. 2N2O5(g) 4NO2 (g) + O2(g) -> and 100 The concentration of N2O5 was measured at regular time intervals and the data presented below [N2O5] (mol/L) 0.1000 Time (s) 0. 0.0707 50 0.0500 100 wll 0.0250 200 0.0125 300 0.00625 400 What is the order of the reaction with respect to N2O5(g)? Justify your answer Give the expression for the rate law Jamnenoo to

3. The gas phase decomposition of N2O5 was studied at a constant temperature. 2N2O5(g) 4NO2 (g) + O2(g) -> and 100 The concentration of N2O5 was measured at regular time intervals and the data presented below [N2O5] (mol/L) 0.1000 Time (s) 0. 0.0707 50 0.0500 100 wll 0.0250 200 0.0125 300 0.00625 400 What is the order of the reaction with respect to N2O5(g)? Justify your answer Give the expression for the rate law Jamnenoo to

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter4: Least-squares And Calibration Methods

Section: Chapter Questions

Problem 6P

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The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by exposure to sunlight for a number of days. One such experiment produced the following results. (Data from R.T. Hedlun and C.R. Youngson, “The Rates of Photodecomposition of Picloram in Aqueous Systems," Fate of Organic Pesticides in tbe Aquatic Environment, Advances in Chemistry Series, #111, American Chemical Society (1972), 159—172.) Exposure Time, t (days) [Pidoram] (mol L_1) 0 4.14 X 10-6 7 3.70 X 10-6 14 3.31 X 10-6 21 2.94 X 10~6 28 2.61 X 10~6 35 2.30 X 10-6 42 2.05 X 10-6 49 1.82 X 10"6 56 1.65 X 10-6 Determine the order of reaction, the rate constant, and the half-life for the photodecomposition of picloram.
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.
Determine the average rate of change of BB from ?=0 st=0 s to ?=272 s.t=272 s. A⟶2BA⟶2B Time (s) Concentration of A (M) 0 0.7300.730 136136 0.4450.445 272272 0.1600.160 rateB= __________M/s
For the decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C2 N2O54 NO2 + O2the following data have been obtained: [N2O5], M 0.603 0.340 0.191 0.108 time, min 0 140 280 420 The average rate of disappearance of N2O5 over the time period from t = 280 min to t = 420 min is ______________ M min-1.
5. At 40oC, H2O2(aq) will decompose according to the equation below:2H2O2(aq)→ 2H2O(l) + O2(g)The following data was collected for the concentration of H2O2 at various times.Time (s) 02.16 x 104 4.32 x 104[H2O2] mol/L 1.0000.500 0.250a) Calculate the average rate of decomposition of H2O2 between 0 and 2.16 x 104 s. Use this to calculate the average rate of production of oxygen gas over the same time.b) What are these rates for the time period from 2.16 x 104 seconds to 4.32 X 104 seconds?
The decomposition of aqueous sucrose to form the isomers glucose and fructose is a common organic reaction, which requires a strong catalyst: C12H22O11(aq) + H2O(l) → 2C6H12O6(aq). The following data were collected during the process: Time (min) [C12H22O11] (mol/L) 0 0.316 39 0.274 80 0.238 140 0.190 210 0.146 (A) If we performed a new trial with an initial concentration of sucrose of 0.400 mol/L, what concentration would remain after 4.0 h has passed?
For the fictitious reaction: AB → A + B Some data was collected measuring the [AB] at certain time intervals. This data was then graphed as described below. A graph of 1/[AB] versus time (s) gives a straight line with the equation: y = 0.0052x + 0.1135 and a R2 = 0.9995. A graph of ln[AB] versus time (s) gives a straight line with the equation: y = -0.0068x + 1.725 and a R2 = 0.8925. Assume the data doesn't fit a zero order reaction. The rate law is: Rate = k[AB]2 Find: What is the value of the rate constant for the given reaction? Select one: a. k = 0.0157 Ms-1 b. k = 0.0052 M-1s-1 c. k = 0.0068 s-1 d. There is no way to determine the value of the rate constant from the given information.
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 -4.34×10-3 min-1 and a y-intercept of -5.20 .Based on this plot, the reaction is _______zerofirstsecond order in SO2Cl2 and the rate constant for the reaction is min-1.
Plot on to graph moles of S2O8 vs time to achieve M/s. The initial concentration of S2O8: 0.05M (added is 2.5mL of 0.200M, but it was diluted so 0.200 x 2.5/10mL = 0.05M). Below is the time (s) and moles consumed. 188s - 0.00002 moles 362s - 0.00004 moles 548s - 0.00006 moles 740s - 0.00008 moles 1001s - 0.0001 moles I was told to plot concentration vs time then subtract the moles, but I'm confused how to do that.
b) what is the velocity of a reaction when [S] = 20 mM, where Vmax = 100 umol/mL*sec, and 4 Km = 2mM? can you show me how he got 98 umol / mL*sec, very close to Vmx, as [S]>>Km, at zero order of the kinetics. step by step please
Use the References to access important values if needed for this question. For the conversion of methyl isonitrile to acetonitrile in the gas phase at 250 °C the following data have been obtained: , M 0.0908 0.0471 0.0244 0.0127 time, s 0 219 438 657 The average rate of disappearance of over the time period from to is M/s . (Please type answer no write by hend)